The moles of potassium chloride needed to make 3M of 0.6L solution is 1.8 moles.
What are moles?The mole designates 6.02214076×10²³ units, which is a very large number. The number of atoms discovered through experimentation to be present in 12 g of carbon-12 was originally used to define the mole. In honour of the Italian physicist Amedeo Avogadro, the number of units in a mole is also known as Avogadro's number or Avogadro's constant (1776–1856). Equal volumes of gases under identical conditions should contain the same number of molecules, according to Avogadro's hypothesis. This idea helped establish atomic and molecular weights and gave rise to the concept of the mole.
What is Avogadro's number?Avogadro's number or Avogadro's constant refers to the quantity of units contained in one mole of any substance. The value is 6.022140857×10²³. Depending on the nature of the reaction and the substance, the units may be electrons, ions, atoms, or molecules.
It links the quantity of substance to the number of particles, bridging the gap between the macroscopic and microscopic worlds.
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if you have a sugar with a molecular weight of 62 g/mol, how many grams would you need to add to 110 ml of water to create a 173 mm solution?
The amount of sugar that you would need to add to 110 ml of water to create a 173 mM solution is 1.17986 grams.
In chemistry, molarity is a measure of the concentration of a solute in a solution. Molarity is usually expressed in moles per liter (M) and is the number of moles of a solute present in a liter of solution. The molarity of a solution is calculated by dividing the number of moles (n) of a solute by the volume (v) of the solution.
M = n/v
When a solution is created, the amount of solute required is determined by the desired molarity of the solution. For instance, if you wanted to create a 173 mM solution, you would need to know the molecular weight (MW) of the solute and the volume of the solution.
n = mass/MW
Combining the two equations, we can solve for the mass using the equation:
mass = n(MW) = M(v)(MW)
Plugging in the values, we get:
Amount of sugar = 173 mM(110 mL)(62 g/mol)
Amount of sugar = 173 x 10⁻³ M(110 mL)(62 g/mol)(1L/1000mL)
Amount of sugar = 1.17986 grams
Therefore, adding 1.17986 grams of sugar to 110 mL of water will create a 173 mM solution.
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a sample of xe takes 75 seconds to effuse out of a container. an unknown gas takes 37 seconds to effuse out of the identical container under identical conditions. what is the most likely identity of the unknown gas?
The most likely identity of the unknown gas that effuses taking 37s is Oxygen(O₂).
Since the unknown gas effuses out faster, it must be lighter than Xe.
The most likely identity of the unknown gas can be determined using Graham's Law of Diffusion. According to this, the time taken for effusion/diffusion of two different gases under identical conditions is directly proportional to the square roots of their densities or molecular masses. It is given as:
t₂/t₁ = √(M₂/M₁)
where t₂,t₁ are the times taken and M₂, M₁ are the molecular masses.
This ratio is determined by the ratio of the molecular weights of the unknown gas and the sample of Xe. The heavier the molecular weight, the slower the rate of effusion.
Rearranging and plugging in the values as t₂= 75s, t₁= 37s, M₁= 131g (for Xe), we get M₂ as follows:
M₂= (37/75)² x 131 = 31.8 ≈ 32g
32g corresponds to the molecular weight of O₂ and it is lighter than Xe.
Therefore, the unknown gas that effuses out of the container faster than the sample of Xe, resulting in the unknown gas taking 37 seconds, and the sample of Xe taking 75 seconds is oxygen(O₂).
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how much oxygen is needed to completely oxidize 1.67*10-3 m glucose solution (c6h12o6) completely to co2 and h2o?
8 moles of oxygen are required to completely oxidize 1.67*10-3 m glucose solution (C6H12O6) completely to CO2 and H2O.
In order to completely oxidize 1.67*10-3 m glucose solution (C6H12O6) completely to CO2 and H2O, 8 moles of oxygen are required.
The balanced equation of the reaction, which is: C6H12O6 + 6O2 ---> 6CO2 + 6H2O.
As there are 6 moles of oxygen molecules on the reactant side, 8 moles of oxygen molecules are needed to completely oxidize 1.67*10-3 m of glucose solution.
This can also be calculated by the equation n=N/V, where n is the molarity of the solution, N is the number of moles of solute and V is the volume of the solution.
Therefore, 8 moles of oxygen is equal to the molarity of the glucose solution multiplied by the volume.
The reaction between oxygen and glucose to form CO2 and H2O is an oxidation reaction. In oxidation reactions, the reactant molecules are oxidized, and as a result, oxygen is reduced.
Therefore, oxygen is needed for the oxidation of glucose molecules to occur. In other words, without the presence of oxygen, the oxidation of glucose to CO2 and H2O cannot occur.
In conclusion, 8 moles of oxygen are required to completely oxidize 1.67*10-3 m glucose solution (C6H12O6) completely to CO2 and H2O.
This can be calculated by the balanced equation of the reaction or by the equation n=N/V. This is an oxidation reaction, meaning oxygen is necessary for the oxidation of glucose molecules to occur.
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upon combustion, a compound containing only carbon and hydrogen produces 2.77 gco2 and 0.851 gh2o . find the empirical formula of the compound.
Answer:Gco is 0.953
Explanation:
in an equilibrium mixture at 500k, the partial pressure of pcl 5 is 0.860 atm, pcl 3 is 0.350 atm, and cl 2 is 1.22 atm. calculate the equilibrium constant (k p ) for this reaction.
0.493 is the equilibrium constant (k p ) for [tex]PCl_5[/tex] (g) ⇌ [tex]PCl_3[/tex] (g) + [tex]Cl_2[/tex] (g) reaction at 500k.
The reaction is given as
[tex]PCl_5[/tex] (g) ⇌ [tex]PCl_3[/tex] (g) + [tex]Cl_2[/tex] (g)
At 500 K, the partial pressure of [tex]PCl_5[/tex] is 0.860 atm, [tex]PCl_3[/tex] is 0.350 atm, and [tex]Cl_2[/tex] is 1.22 atm.
To calculate the equilibrium constant ([tex]K_P[/tex]) for this reaction, we need to use the equation
[tex]K_P[/tex] = [[tex]PCl_3[/tex]] [[tex]Cl_2[/tex]] / [[tex]PCl_5[/tex]]
Here, [[tex]PCl_5[/tex]] = 0.860 atm
[[tex]PCl_3[/tex]] = 0.350 atm
[[tex]Cl_2[/tex]] = 1.22 atm
Substituting these values, we get
[tex]K_P[/tex] = (0.350)(1.22) / 0.860
[tex]K_P[/tex] = 0.493
Therefore, the equilibrium constant ([tex]K_P[/tex]) for this reaction at 500 K is 0.493.
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If I have 28.2 moles of gas at a temperature of 61.8
C, and a volume of 79.2 liters, what is the pressure of the gas in kpa?
The pressure of the 28.2 moles of gas at a temperature of 61.8°C is 991 kPa.
What is the pressure of the gas?Ideal gas law states that "the pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature.
It is expressed as;
PV = nRT
Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant ( 0.08206 Latm/molK )
Given that:
Number of moles n = 28.2
Temperature T = 61.8°C
Volume V = 79.2 L
Pressure P = ?
First, let's convert the temperature from Celsius to Kelvin:
T = 61.8 + 273.15
T = 334.95 K
Now we can plug in the values and solve for P:
P = nRT/V
P = ((28.2 mol) × (0.08206 Latm/molK) × (334.95 K) ) / 79.2 L
P = 9.7866atm
Convert atm to kPa ( multiply the pressure value by 101.3 )
P = 991 kPa
Therefore, the pressure of the gas is 991 kPa.
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Answer:
The pressure of the gas is 991.6 kPa (to the nearest tenth).
Explanation:
To find the total pressure of the gas in kPa, we can use the ideal gas law.
Ideal Gas Law[tex]\boxed{\sf PV=nRT}[/tex]
where:
P is the pressure measured in kilopascal (kPa).V is the volume measured in liters (L).n is the number of moles.R is the ideal gas constant (8.314472 L kPa mol⁻¹ K⁻¹).T is the temperature measured in kelvin (K).Convert the temperature from Celsius to kelvin by adding 273.15:
[tex]\implies \sf 61.8^{\circ}C=61.8+273.15=334.95\;K[/tex]
Therefore, the values are:
V = 79.2 Ln = 28.2 molR = 8.314472 L kPa mol⁻¹ K⁻¹T = 334.95 KSubstitute the values into the formula and solve for P:
[tex]\implies \sf P \cdot 79.2=28.2 \cdot 8.314472 \cdot 334.95[/tex]
[tex]\implies \sf P=\dfrac{28.2 \cdot 8.314472 \cdot 334.95}{79.2}[/tex]
[tex]\implies \sf P=991.60471...[/tex]
[tex]\implies \sf P=991.6\;kPa\;(nearest\;tenth)[/tex]
Therefore, the pressure of the gas is 991.6 kPa (to the nearest tenth).
a certain organic compound contains only c, h, and o. combustion of 0.1000 g of this compound produced 0.2921 g of co2 and 0.0951 g of h2o. what is the empirical formula of the compound?
The empirical formula of the organic compound is C1H1O1 and the simplified form is CHO.
To find the empirical formula of the compound, we need to determine the mole ratios of the elements in the compound.
First, we need to find the number of moles of CO2 and H2O produced by the combustion of 0.1000 g of the compound:
moles of CO2 = 0.2921 g / 44.01 g/mol = 0.006639 mol
moles of H2O = 0.0951 g / 18.02 g/mol = 0.005275 mol
Next, we need to find the number of moles of C and H in the compound. From the combustion reactions, we know that all of the carbon in the compound is converted to CO2, and all of the hydrogens are converted to H2O.
Therefore, the number of moles of C and H in the compound is equal to the number of moles of CO2 and H2O produced, respectively:
moles of C = 0.006639 mol
moles of H = 0.005275 mol
Finally, we need to find the number of moles of O in the compound. We can do this by subtracting the number of moles of C and H from the total number of moles of elements in the compound, which is equal to the mass of the compound divided by its molar mass:
moles of O = (0.1000 g / molar mass of compound) - moles of C - moles of H
The molar mass of the compound is equal to the sum of the molar masses of its constituent elements:
molar mass of compound = molar mass of C + molar mass of H + molar mass of O
Since we don't know the formula of the compound yet, we can assume a generic formula of CxHyOz and calculate the molar mass of this compound as:
molar mass of compound = x(molar mass of C) + y(molar mass of H) + z(molar mass of O)
Using the atomic masses of C, H, and O, we can calculate the molar masses of these elements as:
molar mass of C = 12.01 g/mol
molar mass of H = 1.01 g/mol
molar mass of O = 16.00 g/mol
Substituting these values, we get:
molar mass of compound = 12.01x + 1.01y + 16.00z
Now, we can solve for the number of moles of O in the compound:
moles of O = (0.1000 g / molar mass of compound) - moles of C - moles of H
Substituting the values we found earlier for moles of C and H, we get:
moles of O = (0.1000 g / (12.01x + 1.01y + 16.00z)) - 0.006639 mol - 0.005275 mol
Simplifying, we get:
moles of O = 0.1000 g / (12.01x + 1.01y + 16.00z) - 0.011914 mol
To determine the empirical formula of the compound, we need to find the smallest whole number mole ratio of the elements in the compound. We can do this by dividing the number of moles of each element by the smallest number of moles:
moles of C / 0.005275 = 1.259
moles of H / 0.005275 = 1.000
moles of O / 0.005275 = (0.1000 g / (12.01x + 1.01y + 16.00z) - 0.011914 mol) / 0.005275
Simplifying, we get:
moles of O / 0.005275 = 18.998 - (1.258x + y)
To find the smallest whole number ratio, we can multiply each mole ratio by a common factor that makes the smallest ratio a whole number. In this case, the smallest ratio is 1:1, so we can multiply each ratio by a factor of approximately 0.79 to make the C and H ratios both equal to 1. This gives us:
C: 1.000
H: 0.790
O: 1.484
Since we want whole numbers, we can round these ratios to the nearest whole number, giving us the empirical formula: C1H1O1 or simply CHO.
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If I have 6.00 moles of gas held at a temperature of 93.5 C and in a container with a volume of 41.7 liters, what is the pressure of the gas (ka)?
The pressure of the gas is approximately 4.57 atm or 438.629 kPa
What is the pressure of the gas (ka)?The Ideal gas law or general gas equation states that "the pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature.
It is expressed as;
PV = nRT
Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant ( 0.08206 Latm/molK )
Given that;
P = pressure of the gas (in atm) = ?V = volume of the gas (in L) = 41.7 Ln = number of moles of gas = 6R = the ideal gas constant (0.08206 L.atm/mol.K)T = temperature of the gas (in Kelvin) 93.5°CFirst, we need to convert the temperature to Kelvin:
T (K) = T (Celsius) + 273.15
T (K) = 93.5 + 273.15
T (K) = 366.65 K
Now we can substitute the given values into the formula:
PV = nRT
P = nRT / V
P = ( 6 × 0.08206 × 366.65 ) / 41.7
P = 4.33 atm
Convert to kPa by multiplying the pressure value by 101.3
P = ( 4.33 × 101.3 ) kPa
P = ( 4.33 × 101.3 ) kPa
P = 438.629 kPa
The pressure is approximately 4.57 atm or 438.629 kPa.
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please help the image is attached!!!
Answer:
0.6096
Explanation:
*formula for moles= mass/molormass(RFM)
Molarmass= (28×1)+(19×4)= 104
63.4/104= 0.60961
if the rate constant for a reaction triples when the temperature rises from 25 oc to 65 oc, what is the activation energy of the reaction? give answer in kj/mole.
The activation energy of the reaction, given that the rate constant has tripled when the temperature rose from 25 °C to 65 °C, is 42.6 kJ/mole.
Activation energy is the minimum energy required for a reaction to take place. It is calculated using the Arrhenius equation, which states that the rate constant, k, is proportional to the exponential of negative activation energy (Ea) divided by the gas constant (R) multiplied by the absolute temperature (T).
As the rate constant has tripled when the temperature increased, the activation energy can be calculated as Ea = -R * (1/T2 - 1/T1).
Plugging in the given temperature values of 25 °C and 65 °C and the gas constant, R, the activation energy is 42.6 kJ/mole.
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Calculate the pH of a 0.050 M solution of hydroxylamine, NH2OH. Kb = 6.6 x 10^-9
The pH of hydroxylamine will be 8.76.
The first step is to write the balanced equation for the reaction of hydroxylamine with water:
NH₂OH + H₂O ⇌ NH₃OH⁺ + OH⁻
The Kb expression for this reaction is:
Kb = [NH₃OH⁺][OH⁻] / [NH₂OH]
We are given the Kb value as 6.6 x 10⁻⁹, so we can use this to find the concentration of hydroxylamine that has been deprotonated:
Kb = [NH₃OH⁺][OH⁻] / [NH₂OH]
6.6 x 10⁻⁹ = x² / (0.050 - x)
Assuming that x is very small compared to 0.050, we can simplify the expression as follows:
6.6 x 10⁻⁹ = x² / 0.050
x² = 3.3 x 10⁻¹⁰
x = 5.7 x 10⁻⁶ M
Now that we have the concentration of hydroxide ions, we can use this to find the pH of the solution:
pOH = -log[OH-] = -log(5.7 x 10⁻⁶) = 5.24
pH = 14.00 - pOH = 8.76
Therefore, the pH of a 0.050 M solution of hydroxylamine is 8.76.
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an aqueous potassium carbonate solution is made by dissolving 5.84 5.84 moles of k2co3 k 2 co 3 in sufficient water so that the final volume of the solution is 2.20 l 2.20 l . calculate the molarity of the k2co3 k 2 co 3 solution.
The molarity of the K₂CO₃ solution is 2.65 m.
The molarity of an aqueous potassium carbonate solution can be calculated by using the following formula:
Molarity = moles of solute / liters of solution.
In this case, the moles of solute is 5.84 and the volume of the solution is 2.20 liters. Therefore, the molarity of the potassium carbonate solution is 5.84 moles / 2.20 liters = 2.65 m.
Molarity is an important concept in chemistry and is used to measure the concentration of a solution. Molarity is expressed in terms of moles of solute per liter of solution. In this case, the solution contains 5.84 moles of potassium carbonate per 2.20 liters of water. This makes the molarity of the solution 2.65 m.
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Indicate if the following pairs of compounds could be separated via liquid-liquid extraction.First, draw the structures of the compounds, next determine whether they are acids or bases or neutral. Finally, look up their pKa (or pKb) values and indicate which aqueous solution would separate them or if they are inseparable. Assume that you can utilize aqueous HCl, NaOH, or NaHCO3 for your extractions. For each case that will not work, give the reason.You don't have to draw structure, just explain if they are able to be separated or not and with what and why.1. picric acid and phenol2. salicyclic acid and phenol3. triethylamine and diethylamine4. 3-nitrobenzoic acid and 2-nitrobenzoic acid5. benzylamine and aniline
Picric acid and phenol, Salicylic acid and phenol & Benzylamine and aniline can be separated using liquid-liquid extraction but Triethylamine and diethylamine & 3-nitrobenzoic acid and 2-nitrobenzoic acid cannot be separated using liquid-liquid extraction.
1. Picric acid and phenol can be separated using liquid-liquid extraction. Picric acid is a stronger acid (pKa ~0.4) than phenol (pKa ~10). Adding aqueous NaOH will deprotonate picric acid and make it soluble in the aqueous layer, while phenol remains in the organic layer. Then, the two compounds can be separated.
2. Salicylic acid and phenol can also be separated using liquid-liquid extraction. Salicylic acid (pKa ~3) is more acidic than phenol (pKa ~10). Adding aqueous NaHCO3 will deprotonate salicylic acid, making it soluble in the aqueous layer, while phenol remains in the organic layer. The compounds can then be separated.
3. Triethylamine and diethylamine cannot be easily separated via liquid-liquid extraction, as both are bases (pKb values are similar). Aqueous HCl, NaOH, or NaHCO3 will not be effective in separating these compounds. Alternative separation methods, like distillation, may be needed.
4. 3-nitrobenzoic acid and 2-nitrobenzoic acid cannot be separated using liquid-liquid extraction, as they have similar acidity (pKa values are close) and will react similarly with HCl, NaOH, or NaHCO3. Alternative separation methods, like chromatography, should be considered.
5. Benzylamine and aniline can be separated using liquid-liquid extraction. Benzylamine is a weaker base (pKb ~4.2) than aniline (pKb ~9.4). Adding aqueous HCl will protonate aniline, making it soluble in the aqueous layer, while benzylamine remains in the organic layer. The two compounds can then be separated.
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which of the following substances would undergo dissociation when placed into a polar solvent? question 1 options: c6h12o6 h2o2 mgcl2 co2
The substance that would undergo dissociation when placed into a polar solvent is option C which is MgCl2.
Dissociation explained.
Dissociation refers to the separation of a molecule or compound into smaller particles, such as ions or radicals, usually in a solvent or under the influence of a certain energy input, such as heat or light.
In the context of chemistry, dissociation often refers to the separation of an ionic compound into its constituent ions in a solvent, such as water
MgCl2 is an ionic compound that consists of Mg2+ cations and Cl- anions. When this compound is placed in a polar solvent, such as water, the polar water molecules surround the ions and separate them from one another, resulting in the dissociation of the compound into its constituent ions.
Therefore, other substances listed, C6H12O6 (glucose), H2O2 (hydrogen peroxide), and CO2 (carbon dioxide), are not ionic compounds and do not dissociate into ions when placed in a polar solvent. Glucose and hydrogen peroxide are polar molecules, but they do not ionize in water. Carbon dioxide is a nonpolar molecule and is insoluble in water.
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in which scenario would we be unable to treat the first and second ionization of a diprotic acid as completely separate reactions?
The first and second ionization of a diprotic acid cannot be treated as completely separate reactions when the reaction is taking place in an environment with a fixed pH.
The second ionization of the acid is dependent on the concentration of the ions produced from the first ionization.
If the pH is fixed, then the concentration of the first ionization is also fixed, so the second ionization will not occur completely independently.
For example, a diprotic acid such as oxalic acid can be completely ionized in two steps. In the first ionization, the hydrogen ions of the oxalic acid are replaced with hydroxide ions, forming the oxalate ion:
H2C2O4 + 2H2O → H3O+ + HC2O4–
In the second ionization, the oxalate ion is further dissociated, forming two separate anions and hydronium ions:
HC2O4– + H2O → H3O+ + C2O4–2
However, in an environment with a fixed pH, the second ionization will not take place as the concentration of oxalate ions from the first ionization is fixed.
Therefore, the two ionizations must be treated together in order to accurately predict the final concentrations of the products.
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Answer:
The first ionization constant is greater than the second ionization constant by only a factor of 10.
Explanation:
The two ionization constants must differ by a factor of at least 20 in order to treat the first and second ionizations as chemically (and mathematically) distinct.
onsider a process in which an ideal gas is compressed to one-fourth of its original volume at a constant temperature. calculate the entropy change per mole of gas.
The entropy change per mole of gas is -1.387R.
The entropy change per mole of gas in a process in which an ideal gas is compressed to one-fourth of its original volume at a constant temperature can be calculated as follows:
Let us denote the original volume as V₁, the final volume as V₂, and the number of moles of the gas as n. The entropy change can be calculated using the formula:
ΔS = nR ln (V₂/V₁)
Therefore, the entropy change per mole of gas is given by:
ΔSper mole = R ln (V₂/V₁)
In this case, V₁ = 4V₂ and so,
ΔSper mole = R ln (1/4) = - R ln 4 = -2.303 R log 4 = -1.387R
Thus, the entropy change per mole of gas when an ideal gas is compressed to one-fourth of its original volume at a constant temperature is -1.387R.
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water molecules are attracted to each other and to ions due to . group of answer choices the viscosity of water. electron transfer. electron sharing. surface tension. the polarity of water molecules.
Water molecules are attracted to each other and to ions due to the polarity of water molecules.
The separation of electric charge leading to a molecule having two poles, one positive and the other negative, is referred to as polarity. A polar molecule has a permanent dipole, whereas a nonpolar molecule does not. Water is an example of a polar molecule. The polarity of water is the reason why it is a good solvent and why it is attracted to other polar molecules and ions.
In water, the polar water molecules are pulled toward each other, forming hydrogen bonds. These hydrogen bonds give water its unique properties, such as high surface tension, capillary action, and high boiling and melting points. Ions are also attracted to water due to the polar nature of water molecules. Water molecules surround ions in a process known as hydration or solvation, which stabilizes the ions in solution.
As a result of the polarity of water, it is able to dissolve a wide range of ionic and polar substances, making it one of the most significant substances on the planet.
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which of the following samples has the most moles of the compound? a) 163.0 g of fe2o3 b) 75.0 g of cas c) 150.0 g of bao d) all of the above have the same moles. e) impossible to determine unless the density of each compound is known.
The samples that has the most moles of the compound is option B which is 75.0g
Moles calculation .
To determine which sample has the most moles of the compound, we need to calculate the number of moles of each compound using its molar mass.
a) Fe2O3:
Molar mass of Fe2O3 = 2(55.85 g/mol of Fe) + 3(16.00 g/mol of O) = 159.70 g/mol
Number of moles of Fe2O3 = 163.0 g / 159.70 g/mol = 1.02 mol
b) CaS:
Molar mass of CaS = 40.08 g/mol of Ca + 32.06 g/mol of S = 72.14 g/mol
Number of moles of CaS = 75.0 g / 72.14 g/mol = 1.04 mol
Therefore, sample b) (75.0 g of CaS) has the most moles of the compound, with 1.04 moles. Sample a) (163.0 g of Fe2O3) has 1.02 moles and sample c) (150.0 g of BaO) has 0.98 moles.
So, the correct answer is b.
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A mixture of 90. 0grams of ch4 and 10. Ograms of argon has a pressure of 250 torr under the condition of constant temperature and pressure the partial pressure of ch4 is
The partial pressure of CH₄ in the mixture is 239 torr.
We can use the mole fraction of methane (CH4) to calculate its partial pressure in the mixture. First, we need to convert the masses of each component into moles:
moles of CH₄ = 90.0 g / 16.04 g/mol = 5.61 mol
moles of Ar = 10.0 g / 39.95 g/mol = 0.250 mol
Next, we can calculate the total moles of gas in the mixture,
total moles = moles of CH₄ + moles of Ar = 5.61 mol + 0.250 mol = 5.86 mol
Now we can calculate the mole fraction of CH₄,
mole fraction of CH₄ = moles of CH₄ / total moles = 5.61 mol / 5.86 mol = 0.957
Finally, we can use the mole fraction and total pressure to calculate the partial pressure of CH₄,
partial pressure of CH₄ = mole fraction of CH₄ x total pressure = 0.957 x 250 torr = 239 torr
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what would be the unit of measurement for a surface area that has degrees farenheit as the height and time as the width?
The unit of measurement for a surface area that has degrees Fahrenheit as the height and time as the width would be square degrees Fahrenheit x time.
Surface area is a measurement of the total area that the surface of an object occupies. The surface area is measured in square units. If the surface of an object is rectangular or square, it is calculated by multiplying the length of the object by the width of the object. For the curved surfaces, the formula for the surface area is complicated. However, the concept of square units remains the same for curved surfaces.
Fahrenheit is a unit of temperature that is used to measure the temperature of an object. This is used primarily in the United States and other countries that have adopted the Imperial system of units. It is based on a scale of 180 degrees between the freezing and boiling points of water, where the freezing point is 32°F and the boiling point is 212°F.
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A gas sample at constant pressure and temperature filled with Helium gas had a volume of 221 mL and 4.00 moles. If the volume is increased to 500 ml what is the number of moles of Helium gas that could occupy the container? 0.11 K 9.05 kPa 0.11 kPa 9.05 mol
The number of moles of Helium gas that could occupy the container when the volume is increased to 500 mL is 9.05 mol.
What is the number of moles of the gas?We can use the combined gas law to solve this problem:
(P1 x V1) / (n1 x T1) = (P2 x V2) / (n2 xT2)
where;
P is pressure, V is volume, n is number of moles, and T is temperature.We know that the pressure and temperature are constant, so we can simplify the equation to:
V1/n1 = V2/n2
Solving for n2, we get:
n2 = (V2n1) / V1
Plugging in the values, we get:
n2 = (500 mL * 4.00 mol) / 221 mL
n2 = 9.05 mol
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The diagram shows the cycling of matter in the interior of Earth.
Which statement correctly explains the cycling of matter in the interior of Earth?
Responses
The heat from Earth’s core causes material in the area under the crust to become less dense and rise, while more dense material sinks.
The heat from Earth’s core causes material in the area under the crust to become less dense and rise, while more dense material sinks.
The heat from Earth’s core causes material in the area under the crust to become more dense and rise, while less dense material sinks.
The heat from Earth’s core causes material in the area under the crust to become more dense and rise, while less dense material sinks.
The heat from Earth’s core causes material in the area under the crust to become less dense and sink, while more dense material rises.
The heat from Earth’s core causes material in the area under the crust to become less dense and sink, while more dense material rises.
The heat from Earth’s core causes material in the area under the crust to become more dense and sink, while less dense material rises.
The heat from Earth’s core causes material in the area under the crust to become more dense and sink, while less dense material rises.
Answer:
Explanation:
I think 'The heat from Earth's core causes material in the area under the crust to become denser and rinse, while less dense material sinks.
the energy required to break one mole of iodine-iodine bonds in i2 is 151 kj/mol. what is the longest wavelength of light capable of breaking a single i-i bond?
The longest wavelength of light capable of breaking a single I-I bond is approximately 787 nm (nanometers).
What is energy ?
Energy is considered a quantitative property that can be transferred from an object to perform work.
The energy required to break a mole of I2 molecules is 151 kJ/mol. We can use this information to calculate the energy required to break a single I-I bond:
Energy required to break a single I-I bond = Energy required to break one mole of I2 molecules / Avogadro's number
Energy required to break a single I-I bond = 151 kJ/mol / 6.022 x 10^23 molecules/mol
Energy required to break a single I-I bond = 2.51 x 10^-19 J/bond
To calculate the longest wavelength of light capable of breaking a single I-I bond, we can use the equation:
E = hc/λ
Where
E is the energy of a photon h is Planck's constant c is the speed of lightλ is the wavelength of lightWe want to find the wavelength of light that has an energy of 2.51 x 10^-19 J, so we can rearrange the equation as follows:
λ = hc/E
λ = (6.626 x 10^-34 J s) x (2.998 x 10^8 m/s) / (2.51 x 10^-19 J)
λ = 7.87 x 10^-7 m
Therefore, the longest wavelength of light capable of breaking a single I-I bond is approximately 787 nm (nanometers).
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research a common household chemical, a cosmetic compound, a medical drug, or something else that is commonly known and find out what its chemical name is.
The chemical name of water is hydrogen oxide.
Water is a compound with the chemical name hydrogen oxide (H2O).
It is a colorless, odorless, and tasteless liquid that is essential for most forms of life on Earth.
Water is a chemical molecule; therefore, its many forms have different names depending on their individual constituents. According to the nomenclature established by the IUPAC, water may alternatively be referred to as dihydrogen monoxide, dihydrogen oxide, hydrogen hydroxide, or hydric acid.
Being the primary component of Earth's hydrosphere and the fluids of all known forms of life, water (chemical formula H 2 O) is an inorganic, clear, tasteless, odorless, and almost colorless chemical substance (in which it acts as a solvent). None of the known forms of life could survive without it, despite the fact that it offers neither dietary energy nor organic micronutrients.
Water is made up of two hydrogen atoms and one oxygen atom, with the formula H2O.
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which of the combinations below will produce an insoluble salt? a) ba(oh)2 hcl b) mnso4 pb(no2)2 c) h2so4 albr3
The combination that will produce an insoluble salt is b) MnSO4 Pb(NO2)2.
A salt is a chemical compound made up of cations (positively charged ions) and anions (negatively charged ions) (negatively charged ions). The ions must be combined in such a way that the sum of the charges is zero. NaCl is the most well-known saltand it is made up of sodium cations (Na+) and chloride anions (Cl-).MnSO4 Pb(NO2)2 is the answer since both of these elements are soluble. MnSO4 is a soluble substance that is sometimes used in the production of ceramics.
MnSO4 is often used as a nutritional supplement for animals since it is a good source of manganese. Pb(NO2)2 is a powder that is bright yellow, it has a molar mass of 325.2 g/mol. It is made up of two NO2 anions (negatively charged ions) and one Pb2+ cation (positively charged ion).The formation of insoluble salts can occur when the cations and anions in a reaction solution bind to create a new solid. Since the newly formed solid is insoluble, it settles to the bottom of the solution and can be separated from the liquid through filtration. The insoluble salt that is formed is a white or colorless substance that appears as a powder.
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How many grams are in 87g of potassium bromide?
The number of mole present in 87 grams of potassium bromide, KBr is 0.731 mole
How do i determine the number of mole present?We'll begin our calculation by obtaining the molar mass of potassium bromide, KBr. Details below:
Molar mass of ptassium, K = 39 g/molMolar mass of bromine, Br = 80 g/molMolar mass of potassium bromide, KBr =?Molar mass of potassium bromide, KBr = K + Br
Molar mass of potassium bromide, KBr = 39 + 80
Molar mass of potassium bromide, KBr = 119 g/ mol
Finally, we shall determine the number of mole present. Details below:
Mass of potassium bromide, KBr = 87 grams Molar mass of potassium bromide, KBr = 119 g/mol Mole of potassium bromide, KBr =?Mole = mass / molar mass
Mole of potassium bromide, KBr = 87/ 119
Mole of potassium bromide, KBr = 0.731 mole
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Complete question:
How many moles are in 87g of potassium bromide?
a solution of cacl2 cacl 2 in water forms a mixture that is 31.5% 31.5 % calcium chloride by mass. if the total mass of the mixture is 195.4 g, 195.4 g, what masses of cacl2 cacl 2 and water were used?
The masses of calcium chloride (CaCl2) and water used to form the mixture are 61.18 g and 134.22 g, respectively.
The mass of calcium chloride (CaCl2):
The percentage of calcium chloride (CaCl2) in the mixture is 31.5%.
Multiply the total mass of the mixture (195.4 g) by 31.5% to find the mass of calcium chloride (CaCl2) in the mixture:
Mass of calcium chloride (CaCl2) = (195.4 g) x (31.5%) = 61.18 g
The mass of water:
Subtract the mass of calcium chloride (CaCl2) from the total mass of the mixture (195.4 g) to find the mass of water in the mixture:
Mass of water = (195.4 g) - (61.18 g) = 134.22 g
Therefore, masses of calcium chloride (CaCl2) and water used to form the mixture are 61.18 g and 134.22 g, respectively.
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as the temperature increases, the rate of enzymatic reactions can ; however, at extremely high temperatures (95c) the rate will dramatically due to .
As the temperature increases, the rate of enzymatic reactions generally increases as well, because the molecules have more kinetic energy and collide more frequently.
What are enzymes?Enzymes are proteins with specific three-dimensional shapes that are critical to their function. At high temperatures, the increased kinetic energy can disrupt the weak forces that hold the protein's structure together, causing the enzyme to lose its shape and become denatured. Denatured enzymes can no longer bind to substrates, and the rate of enzymatic reactions will drop sharply.
The temperature at which an enzyme denatures depends on the specific enzyme and its optimal temperature range. Some enzymes are adapted to function at very high temperatures, such as those found in thermophilic bacteria that live in hot springs or hydrothermal vents.
However, most enzymes have a more narrow temperature range within which they can function optimally, and extreme temperatures can cause irreversible damage to the enzyme structure.
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4. a laboratory experiment calls for 0.150 m hno3. what volume of 0.150 m hno3 can be prepared form 0.350 l of 1.98 m hno3?
The volume of 0.150 M HNO3 that can be prepared from 0.350 L of 1.98 M HNO3 is 0.07112 L, or approximately 71.12 mL (since 1 L = 1000 mL).
The given equation is used to calculate the volume (V1) of a desired concentration of a solution (0.150 M HNO3) that can be prepared from a given volume (V2) of a known concentration solution (1.98 M HNO3), using the ratios of their concentrations (C1 and C2).
Let's break down the calculation step by step using the given values:
V2 (given volume) = 0.350 L
C1 (desired concentration) = 0.150 M
C2 (known concentration) = 1.98 M
Plugging these values into the equation, we get:
V1 (0.150 M HNO3) = V2 (1.98 M HNO3) x (C1 (0.150 M) / C2 (1.98 M))
V1 = 0.350 L x (0.150 M / 1.98 M)
V1 = 0.350 L x 0.0758
V1 = 0.07112 L
Therefore, the volume of 0.150 M HNO3 that can be prepared from 0.350 L of 1.98 M HNO3 is 0.07112 L, or approximately 71.12 mL (since 1 L = 1000 mL).
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which process has the larger entropy change: melting ice or boiling water? which process has the larger entropy change: melting ice or boiling water? melting ice boiling water g
Boiling water has a larger entropy change compared to melting ice. Entropy is a gauge of a system's unpredictability or disorder. A substance's particles have more flexibility to move when it changes from a solid to a liquid or from a liquid to a gas, which causes an increase in disorder and unpredictability. This rise in entropy often follows the rise in molecular randomness.
When ice melts, the arrangement of its particles changes from one that is more structured and organized in the solid state to one that is more random and disordered in the liquid state. Entropy rises as a result of this.
The arrangement of the particles changes from being very tightly packed in the liquid form of water to being much more dispersed and randomly distributed in the gas state as it boils and turns into steam. Compared to ice melting, this increase in volume and the particles' ability to move about causes a far bigger increase in entropy.
In conclusion, melting ice causes a smaller rise in entropy than boiling water does because gaseous particles are more dispersed and random than liquid ones.
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