[tex] \ddots[/tex] The heat energy can be deduced as -
[tex] \odot\sf \footnotesize{Heat \:energy = Mass\: of\: substance\times Specific \:heat\times Change\: in \:temperature}\\[/tex]
[tex] \qquad :\implies\sf \boxed{\sf Q = mS\Delta T}\\[/tex]
Where-
Q = Heat energy (Joules, J)m = Mass of a substance (g or,kg) S = Specific heat ( J/g∙°C or, J/kg.°C)For liquid water, this value is 4.18J/g∙°C∆ is a symbol meaning "the change in"∆T = Change in temperature (Kelvins, K)In this instant, we are given -
Heat energy,Q = 14.5 KJ = 14500JMass of substant, m = 485 g[tex] \ddots[/tex] Now that we have all the required values except ∆T,so we can plug the rest of the known values into the formula and solve for ∆T -
[tex] \qquad :\implies\sf \underline{Q = mS\Delta T}\\[/tex]
[tex] \qquad :\implies\sf 14500 = 485 \times 4.18 \times \Delta T\\[/tex]
[tex] \qquad :\implies\sf 14500 = 2027.3\times \Delta T\\[/tex]
[tex] \qquad :\implies\sf \Delta T = \dfrac{14500}{2027.3}\\[/tex]
[tex] \qquad :\implies\sf \Delta T = 7.152370........\:°C\\[/tex]
[tex] \qquad :\implies\sf \underline{\boxed{\sf \Delta T=7.15\:°C}}\\[/tex]
[tex] \ddots[/tex]Correct answer - [tex]\boxed{\sf \Delta T=7.15\:°C}.[/tex]
This is an exercise in specific heat and thermal conductivity which are two important physical properties that describe how materials interact with heat. Specific heat refers to the amount of energy required to raise the temperature of a material by a given amount, while thermal conductivity refers to a material's ability to transfer heat through itself.
The formula for specific heat is Q = mcΔT, where Q is the amount of heat transferred, m is the mass of the material, c is the specific heat, and ΔT is the change in temperature. The unit of measure for specific heat is J/(g*°C).
On the other hand, thermal conductivity is measured in terms of the amount of heat that is transferred through a material per unit time and area, given a temperature difference. It is expressed as the amount of heat transferred per second, per square meter, per meter of material thickness, when the temperature difference between the extremes is one Kelvin. Its formula is Q/t = -kA(∆T/∆x), where Q/t is the heat transfer rate, k is the thermal conductivity, A is the cross-sectional area, ∆T is the temperature difference, and ∆ x is the thickness of the material.
These properties are useful for understanding how materials interact with heat in a variety of situations, from building design to heating and cooling equipment manufacturing.
We solve the exercise, for the temperature change:
Now to calculate the temperature rise of 485 g of liquid water when 14.5 kJ of heat is added to it, we can use the formula:
Q = mcΔT
We must know that it has a quantity of heat of 14.5 Kj, with a mass of 485 g. The specific heat capacity of water is 4.18 J/(g °C).
First, we need to convert the heat added to joules:
Q = 14.5 KJ × (1000 J/1 KJ)
Q = 14500 J
We can then solve for ΔT. We clear the formula.
ΔT = Q / (m × c)
We substitute our data in the formula and solve the temperature change:
ΔT = Q / (m × c)
ΔT = (14500 J)/(485 g × 4.18 J/(g·°C))
ΔT ≈ 7.15 °C
The water would increase its temperature by approximately 7.15°C if 14.5 kJ of heat were added.
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Which statement about the reaction between calcium oxide and water is correct?
a) 65.2 kJ of heat are released for every mole of CaO that reacts.
b) 130 kJ of heat are released for every mole of H2O that reacts.
c) 130 kJ of heat are absorbed for every mole of CaO that reacts.
d) 65.2 kJ of heat are absorbed for every mole of H2O that reacts.
The heat that is released is 1600 J
65.2 kJ of heat are released for every mole of CaO that reacts.
What is the heat released?For every mole of CaO that combines with water, 65.2 kJ of heat are generated, according to thermodynamic statistics. As a result, a considerable amount of heat is emitted throughout the reaction, making it highly exothermic.
We know that;
H = mcdT
H = heat absorbed or evolved
m = mass of the substance
c = Heat capacity of the substance
dT = temperature change.
H = 60 * 1 * (43 - 70)
H = -1600 J
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The volume of a sample of oxygen is 200.0 mL when the pressure is 3.000 atm and the temperature is 37.0 C. What is the new temperature if the volume increases to 400.0 mL and the pressure decreases to 2.000 atm?
Answer:
140.3 *C
Explanation:
(P1 * V1) / T1 = (P2 * V2) / T2
where P1 = 3.000 atm, V1 = 200.0 ml, T1 = 37.0°C + 273.15 = 310.15 K, P2 = 2.000 atm, V2 = 400.0 ml.
Substituting these values into the formula gives:
(3.000 atm * 200.0 ml) / 310.15 K = (2.000 atm * 400.0 ml) / T2
Solving for T2 gives:
T2 = (2.000 atm * 400.0 ml * 310.15 K) / (3.000 atm * 200.0 ml)
T2 ≈ 413 K or 140°C.
Select all the elementary substances.
silver bromide (AgBr)
silicon dioxide (SiO₂)
hydrogen sulfide (H₂S)
xenon (Xe)
Answer:
silicon dioxide,xenon
Explanation:
For the reaction: N₂(g) + 3H₂(g) + 2NH3(g) AH = -76.4 KJ/mol. Determine the heat energy when 5.0g of hydrogen burns.
Answer:
-191 kJ
Explanation:
The given reaction is:
N₂(g) + 3H₂(g) → 2NH₃(g) ΔH = -76.4 kJ/mol
From the balanced equation, we can see that the stoichiometric ratio between hydrogen (H₂) and ammonia (NH₃) is 3:2. This means that 3 moles of hydrogen react to produce 2 moles of ammonia.
To determine the heat energy when 5.0 g of hydrogen (H₂) burns, we need to follow these steps:
Step 1: Calculate the moles of hydrogen (H₂)
Using the molar mass of hydrogen (H₂), which is 2 g/mol, we can calculate the moles of hydrogen (H₂) in 5.0 g of hydrogen:
Moles of H₂ = Mass of H₂ / Molar mass of H₂
Moles of H₂ = 5.0 g / 2 g/mol
Moles of H₂ = 2.5 mol
Step 2: Use the stoichiometry of the reaction
Based on the stoichiometry of the reaction, we know that 3 moles of hydrogen (H₂) react to produce 2 moles of ammonia (NH₃), and the enthalpy change (ΔH) is -76.4 kJ/mol.
Step 3: Calculate the heat energy
The heat energy for 2.5 moles of hydrogen (H₂) can be calculated using the given enthalpy change (ΔH) and the stoichiometry of the reaction:
Heat energy = Moles of H₂ x ΔH
Heat energy = 2.5 mol x -76.4 kJ/mol
Heat energy = -191 kJ (rounded to three significant figures)
So, the heat energy when 5.0 g of hydrogen (H₂) burns is -191 kJ (rounded to three significant figures), and the negative sign indicates that the reaction is exothermic, releasing heat.
When dinitrogen pentoxide is heated, it decomposes to
nitrogen dioxide and oxygen. How many moles of nitrogen
dioxide can be formed from the decomposition of 1.25 g of
dinitrogen pentoxide?
The process decomposes dinitrogen pentoxide into nitrogen dioxide and oxygen. The reaction has a rate constant of 5.8103/s (5.8 10 3 / s).
Does the breakdown of N₂O₅and N₂O follow first order kinetics?According to the process described below, the thermal breakdown of N₂O₅ follows first order kinetics: N₂O₅→2NO₂+12O₂. Find the rate constant of the reaction if the starting pressure of N₂O₅ is 100 mm and the pressure created after 10 minutes is 130 mm.
The breakdown of N₂O₅ according to the equation: 2N₂O₅ (g)4NO₂(g)+O₂(g) is a first-order reaction. After 30 minutes of decomposition in a closed vessel, the total pressure created is 284.5 mm of Hg, and after full decomposition, the total pressure is 584.5 mm of Hg.
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35.0 ml. of a 0.250 M solution of /OH is titrated with 0.150 M HCI. After 35.0 mL of the HCl has been added, the resultant
Determine the amount of KOH present in the resulting solution. KOH was initially 0.00875 mol, then 0.00525 mol of it interacted with HCl. As a result, 0.00875 mole - 0.00525 mol (= 0.00350 mol of KOH is left. The resulting solution has a volume of 70.0 mL (35.0 mL plus 35.0 mL).
Is HCl directly titrated with NaOH?The titrant (NaOH), which is added gradually throughout the course of a titration, is added to the unknown substance. The equivalency point is the moment at which precisely the right quantity of titrant (NaOH) has indeed been added that react to the entire analyte (HCl).
What happens when you titrate NaOH to HCl?What took place during titration: One mole of NaOH interacts with one mole of HCl inside the reaction between the two substances. NaOH with HCl equals NaCl plus H2O. (NaOH and HCl have a mole ratio of 1:1.) • The NaOH concentration is 0.1 M, or 0.1 molecules per litre.
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Calculate the cell potential, Ecell, for the following reaction at 298k.
Co(s)+2Ag+(0.010M)=Co+2(0.015M)+2 Ag(s)
To calculate the cell potential, Ecell, for the given reaction at 298K, we need to use the Nernst equation. The Nernst equation relates the cell potential to the standard cell potential, temperature, and the concentrations of the reactants and products. The Nernst equation is given as follows:
Ecell = E°cell - (RT/nF) ln(Q)
where,
Ecell = cell potential
E°cell = standard cell potential
R = gas constant (8.314 J/K.mol)
T = temperature (298 K)
n = number of electrons transferred in the balanced redox reaction
F = Faraday constant (96,485 C/mol)
Q = reaction quotient
The given reaction is a redox reaction, which involves the transfer of two electrons from Co to Ag+. The balanced half-reactions are as follows:
Co(s) → Co2+(aq) + 2 e-
Ag+(aq) + e- → Ag(s)
The standard reduction potentials for these half-reactions are:
Co2+(aq) + 2 e- → Co(s) E°red = -0.28 V
Ag+(aq) + e- → Ag(s) E°red = +0.80 V
The overall standard cell potential can be calculated by subtracting the standard reduction potential of the anode from that of the cathode:
E°cell = E°red,cathode - E°red,anode
= +0.80 V - (-0.28 V)
= +1.08 V
Now we need to calculate the reaction quotient Q using the concentrations of the reactants and products. According to the given information, [Ag+] = 0.010 M and [Co2+] = 0.015 M.
Q = ([Co2+][Ag+]^2)/([Ag+]^2)
= ([0.015][0.010]^2)/([0.010]^2)
= 0.015 M
Substituting the values in the Nernst equation, we get:
Ecell = E°cell - (RT/nF) ln(Q)
= 1.08 - (8.314 x 298 / (2 x 96485)) ln(0.015)
= 0.829 V
Therefore, the cell potential, Ecell, for the given reaction at 298K is 0.829 V.
Consider the reaction described by the chemical equation shown.
C2H4(g)+H2O(l)⟶C2H5OH(l)Δ∘rxn=−44.2 kJ
Use the data from the table of thermodynamic properties to calculate the value of Δ∘rxn
at 25.0 ∘C.
ΔS∘rxn= ? J⋅K−1
Calculate Δ∘rxn.
ΔG∘rxn= ? kJ
In which direction is the reaction, as written, spontaneous at 25 ∘C
and standard pressure?
reverse
both
neither
forward
Answer:
To calculate Δ∘rxn, we can use the following formula:
ΔG∘rxn = ΔH∘rxn - TΔS∘rxn
where ΔH∘rxn is the enthalpy change of the reaction, T is the temperature in Kelvin, and ΔS∘rxn is the entropy change of the reaction.
We know that ΔH∘rxn = -44.2 kJ and we want to find ΔS∘rxn at 25.0 ∘C (298 K). We can use the following formula to calculate ΔS∘rxn:
ΔG∘rxn = -RTlnK
where R is the gas constant (8.314 J/mol K), T is the temperature in Kelvin, and K is the equilibrium constant.
We can find K using the following formula:
ΔG∘rxn = -RTlnK K = e^(-ΔG∘rxn/RT)
We know that ΔG∘rxn = -44.2 kJ/mol and R = 8.314 J/mol K, so we can calculate K:
K = e^(-(-44.2 kJ/mol)/(8.314 J/mol K * 298 K)) K = 1.9 x 10^7
Now we can use K to calculate ΔS∘rxn:
ΔG∘rxn = -RTlnK ΔS∘rxn = -(ΔH∘rxn - ΔG∘rxn)/T ΔS∘rxn = -((-44.2 kJ/mol) - (-8.314 J/mol K * 298 K * ln(1.9 x 10^7)))/(298 K) ΔS∘rxn = -0.143 kJ/K
Therefore, ΔS∘rxn is -0.143 kJ/K.
To determine whether the reaction is spontaneous at 25 ∘C and standard pressure, we can use Gibbs free energy (ΔG). If ΔG < 0, then the reaction is spontaneous in the forward direction; if ΔG > 0, then it is spontaneous in the reverse direction; if ΔG = 0, then it is at equilibrium.
We know that ΔG∘rxn = -44.2 kJ/mol and T = 25 ∘C (298 K). We can use the following formula to calculate ΔG:
ΔG = ΔG∘ + RTlnQ
where Q is the reaction quotient.
At equilibrium, Q = K (the equilibrium constant). Since we calculated K earlier to be 1.9 x 10^7, we can use this value for Q.
ΔG = ΔG∘ + RTlnQ ΔG = (-44.2 kJ/mol) + (8.314 J/mol K * 298 K * ln(1.9 x 10^7)) ΔG = -43.6 kJ/mol
Since ΔG < 0, the reaction is spontaneous in the forward direction at 25 ∘C and standard pressure.
whats the answer and why?
I would say C
Since the nitro group (NO2) contains a positively charged nitrogen atom, it tends to attract electron from the aromatic ring and, therefore, the other group/atom. In the first case, I think piridine (II) makes a stronger bond with water since the nitrogen in the aromatic ring needs its electrons in order to be have a slight negative charge that can interact with the slightly positive charged hydrogen atom in water. If the nitro group is present, it will attract to some extent the electrons of the nitrogen atom in the ring, thus making the H-bond less stronger.
In the second case the hydrogen, which is slightly positive, of the OH group interacts with the oxygen, which is slightly negative, of water. If the nitro group is present, it will attract the electrons of oxygen of the hydroxyl group, therefore making the bond between the oxygen and the hydrogen more polar (which basically means that the bonding electron of hydrogen is even more attracted by the oxygen atom) making the hydrogen atom more positive, which means that the H-bond will be stronger
Question 4 of 10
How much energy is required to vaporize 2 kg of gold? Use
the table below and this equation: Q = mLvapor
Substance
Aluminum
Copper
Gold
Helium
Lead
Mercury
Water
Latent Heat
Fusion
(melting)
(kJ/kg)
400
207
62.8
5.2
24.5
11.4
335
Melting
Point
(°C)
660
1083
1063
-270
327
-39
0
Latent Heat
Vaporization
(boiling) (kJ/kg)
1100
4730
1720
21
871
296
2256
Boiling
Point
(°C)
2450
2566
2808
-269
1751
357
100
It requires 10.15 kilojoules of energy.
What is vaporization?The term "vaporisation" (or "evaporation") often refers to the transformation of a liquid's condition into a vapour phase below its boiling point. The phrase, however, can also refer to the process of removing a solvent, independent of the temperature used.
What is energy?When a body moves to exert force, it is said to be exerting work. Energy is the capacity to accomplish work. Energy is something we always need, and it can take many different forms.
If the gold is present in the liquid state, you only have to determine the latent heat of vaporization, or lvap. The empirical data for gold is 330 kJ/mol.
Q = mlvap
Q = (2 kg)(1 kmol/197 kg)(1,000 mol/1 kmol)
Q = 10.15 kJ
It needs an energy of 10.15 kilojoules
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Is a sample of oxygen gas at 70 degrees celsius
twice as hot as a sample of oxygen gas at 35 degrees celsius
A sample of oxygen gas at 70 degrees Celsius is not twice as hot as a sample of oxygen gas at 35 degrees Celsius.
What is Temperature?
Temperature is a physical property that describes the degree of hotness or coldness of a substance, typically measured with a thermometer in units such as Celsius or Fahrenheit. It is a measure of the average kinetic energy of the particles that make up a substance, with higher temperatures indicating greater kinetic energy and lower temperatures indicating less kinetic energy.
The temperature difference between the two samples is 35 degrees Celsius, not 70 degrees Celsius. Temperature is a measure of the average kinetic energy of the particles in a substance, and it is on an absolute scale (Kelvin).
As we can see, the temperature in Kelvin of oxygen gas at 70 degrees Celsius (343.15 K) is not twice the temperature of oxygen gas at 35 degrees Celsius (308.15 K). Therefore, a sample of oxygen gas at 70 degrees Celsius is not twice as hot as a sample of oxygen gas at 35 degrees Celsius.
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Your conclusion will include a summary of the lab results and an interpretation of the results.
Please answer all questions in complete sentences using your own words.
1. Identify the independent variable?
2. Identify the dependent variable?
3. Why do you believe knowing how elements and compounds react together is essential in
everyday matters?
I
4. Choose one of the compounds from the table and explain how you know the number of
atoms in your formula.
5. Is it possible for two different compounds to be made from the same two elements? Why
or why not?
6. With a limited number of elements (less than 120 are known), does this mean we also
have a small number of compounds? Or do we have many compounds in this world?
The independent and dependent variables are compounds and elements, respectively.
Why do you believe knowing how elements and compounds react together is essential in everyday matters?Elements and compounds make up everything in our surroundings. Knowing how things operate can aid in our ability to comprehend our surroundings.
Explain how you determined the number of atoms in your formula for one of the compounds in the table.Water is one of the chemicals listed in the table (H2O). This molecule has 3 atoms, which can be broken down into 2 hydrogen (H) atoms and 1 oxygen atom (O).
Can the same two elements be combined to form two distinct compounds? If not, why not?Several compounds can be created by mixing the same two elements' atoms in different ratios.
Does having a minimal number of known elements (less than 120) imply that there aren't many compounds as well? Or does this universe contain a lot of compounds?Because these elements mix in various ways and in various quantities to create unique compounds, we have a huge variety of compounds in this universe.
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PLS HELPPPPPP
how many grams of iron are present in 9.24x10^22 atoms of Fe?
The mass of iron present in 9.24 x [tex]10^{22}[/tex] atoms of Fe is approximately 0.852 grams.
What is Molar Mass?
Molar mass is the mass of one mole of a substance, expressed in grams per mole. It is calculated by summing the atomic masses of all the atoms in a molecule or formula unit.
The molar mass of iron (Fe) is approximately 55.85 g/mol. We can use this to convert the number of atoms of Fe to the mass of Fe.
First, we can calculate the number of moles of Fe in 9.24x[tex]10^{22}[/tex] atoms:
Mass of Fe = 9.24 x [tex]10^{22}[/tex] atoms x 55.845 g/mol / 6.022 x [tex]10^{-23}[/tex]atoms/mol
Mass of Fe = 0.852 g
So, the mass of iron present in 9.24 x [tex]10^{22}[/tex] atoms of Fe is approximately 0.852 grams.
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For the equilibrium mixture:
NH4Cl(s) + heat <=> NH4+(aq) + Cl-(aq)
A) What change do you observe when you add concentrated hydrochloric acid, HCl, solution. Give complete explanation.
The addition of concentrated HCl to the equilibrium mixture will result in the precipitation of more NH₄Cl(s) as the equilibrium shifts towards the left. This can be observed as cloudiness or precipitation forming in the solution.
When concentrated hydrochloric acid (HCl) solution is added to the equilibrium mixture of NH₄Cl(s) + heat <=> NH₄+(aq) + Cl-(aq), the equilibrium will shift towards the left, meaning more solid NH₄Cl will be formed.
This is because HCl is a strong acid that will react with NH₄+ ion to form NH₄Cl(s) and H+ ion:
NH₄+(aq) + Cl-(aq) + HCl(aq) → NH₄Cl(s) + H₂O(l)
The increase in H+ ion concentration due to the addition of HCl will result in the shift of the equilibrium to the left to reduce the excess H+ ion concentration. This will favor the formation of more solid NH₄Cl.
Therefore, the addition of concentrated HCl to the equilibrium mixture will result in the precipitation of more NH₄Cl(s) as the equilibrium shifts towards the left. This can be observed as cloudiness or precipitation forming in the solution.
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Sulfur reacts with oxygen gas to form sulfur dioxide gas according to the following reaction. S8(s)+8O2(g)⟶8SO2(g). For this reaction, ΔH=−2374 kJ and ΔS=312.2 J/K. Calculate ΔG for this reaction at 805 K.
The reaction's G value at 805 K is -2625.7 kJ.
Sulphur dioxide gas is the name of the byproduct created when sulphur and gas react.Sulfur dioxide gas is the byproduct of the interaction between sulphur and oxygen. Sulphurous acid is created when sulphur dioxide dissolves in water. Sulfuric acid causes blue litmus paper to turn red. Non-metal oxides typically have an acidic character.
ΔG = ΔH - TΔS
where ΔH is the enthalpy change, ΔS is the entropy change, T is the temperature in Kelvin, and ΔG is the change in Gibbs free energy.
Substituting the given values:
ΔG = -2374 kJ - (805 K)(312.2 J/K)
ΔG = -2374 kJ - 251717 J
ΔG = -2374 kJ - 251.7 kJ
ΔG = -2625.7 kJ
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2. When dinitrogen pentoxide is heated, it decomposes to
nitrogen dioxide and oxygen. How many moles of nitrogen
dioxide can be formed from the decomposition of 1.25 g of
dinitrogen pentoxide?
0.02314 moles of NO₂ can be formed from the decomposition of 1.25 g of dinitrogen pentoxide.
The balanced equation for the decomposition of dinitrogen pentoxide is:
2 N₂O₅ → 4 NO₂ + O₂
The molar mass of N₂O₅ is 108.01 g/mol.
To determine the number of moles of N₂O₅ present in 1.25 g, we use the following calculation:
moles N₂O₅ = mass / molar mass
moles N₂O₅ = 1.25 g / 108.01 g/mol
moles N₂O₅ = 0.01157 mol
From the balanced equation, we can see that 2 moles of N₂O₅ decompose to form 4 moles of NO2. Therefore, the number of moles of NO2 produced can be calculated as:
moles NO₂ = (0.01157 mol N2O5) × (4 mol NO2 / 2 mol N2O5)
moles NO₂ = 0.02314 mol
Therefore, 0.02314 moles of NO₂ can be formed from the decomposition of 1.25 g of dinitrogen pentoxide.
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A mixture that contains large particles that are uniformly dispersed is called a _____.
solvent
emulsion
alloy
colloid
Answer:
colloid
Explanation:
there's no explanation
Determine the molarity (M) of 0.2074 g of calcium hydroxide, Ca(OH)₂ (74.09 g/mol), in 40.00 mL of solution.
Answer:
M=0.06998 mol/L
Explanation:
The temperature of a 2.0-liter sample of helium gas at STP is increased to 27C, and the pressure is decreased to 80 kPa. What is the new volume of the helium sample? Round your answer to the nearest tenth of a liter?
The new volume of the helium sample would be 2.4 L.
Volume of a gasAccording to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in kelvins.
At STP (standard temperature and pressure), which is defined as 0°C (273.15 K) and 101.325 kPa, the volume of 2.0 liters of helium gas contains one mole of helium atoms.
To find the new volume of the helium sample when the temperature is increased to 27°C (300.15 K) and the pressure is decreased to 80 kPa, we can use the following equation:
(P1V1)/T1 = (P2V2)/T2
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.
Plugging in the values, we get:
(101.325 kPa)(2.0 L)/(273.15 K) = (80 kPa)(V2)/(300.15 K)
Solving for V2, we get:
V2 = (101.325 kPa)(2.0 L)/(273.15 K) * (300.15 K)/(80 kPa) = 2.36 L
Therefore, the new volume of the helium sample is approximately 2.4 L (rounded to the nearest tenth).
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50 points +brainlist (there's going to be 3 more added on my profile with the same points(
which type of process is this?
chemical
physical
nuclear
nuclear type of process is this
Is the reaction physical or chemical?The content of a physical reaction differs from that of a chemical reaction. A chemical reaction changes the makeup of the substances in question; a physical change changes the look, smell, or plain presentation of a sample of matter without changing its content.
Nuclear reactions are not the same as chemical reactions. Atoms become more stable in chemical processes by engaging in electron transfers or by sharing electrons with other atoms.
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8. Balance the following equation:
NH3(g) + F2(g) → N₂F4(g) + HF(g)
a. How many moles of each reactant are needed to produce 4.00 moles of HF?
b. How many grams of F2 are required to react with 1.50 moles of NH3?
c. How many grams of N₂F4 can be produced when 3.40 grams of NH3 reacts?
Answer:
2NH₃(g) + 5F₂(g) → N₂F₄(g) + 6HF(g)
(a) mol of NH₃ required = 1.333 mol; mol of F₂ required = 3.333 mol
(b) mass of F₂ required = 142.5 g
(c) N₂F₄ produced = 10.38 g
Explanation:
2NH₃(g) + 5F₂(g) → N₂F₄(g) + 6HF(g)
What is Stoichiometry?
In chemical equations, unless stated otherwise, the reactants and products will theoretically always remain in stoichiometric ratios.
The stoichiometry of a reaction is the relationship between the relative quantities of products and reactants, typically a ratio of whole integers.
Consider the following chemical reaction: aA + bB ⇒ cC + dD.
The stoichiometry of reactants to products in this reaction is the ratio of the coefficients of each species: a : b : c : d.
Converting between moles and mass:
To convert from mass to moles, divide the mass present by the molar mass, resulting in the number of moles.
Thence, the formula for moles: n = m/M, where n = number of moles, m = mass present, and M = molar mass. This formula can be easily rearranged to find mass present from molar mass and moles, or molar mass from mass and moles.
a. How many moles of each reactant are needed to produce 4.00 moles of HF?
In the given chemical equation, the stoichiometry of the reaction is
2 : 5 : 1 : 6. Therefore, for every 2 moles of NH₃, we require 5 moles of F₂, which will produce 1 mole of N₂F₄ and 6 moles of HF.
mol of NH₃ required = 1/3 × mol of HF = 1.333 mol
mol of F₂ required = 5/6 × mol of HF = 3.333 mol
b. How many grams of F₂ are required to react with 1.50 moles of NH₃?
Using stoichiometry again: mol of F₂ required = 5/2 × mol of NH₃
∴ F₂ required = 3.75 mol.
Then we can convert this to mass: m = nM = (3.75)(2×19.00) = 142.5 g
c. How many grams of N₂F₄ can be produced when 3.40 grams of NH₃ reacts?
Converting mass to moles: n = m/M = 3.40/(14.01+1.008×3) = 0.1996 mol
Using stoichiometry again: mol of N₂F₄ produced = 1/2 × mol of NH₃
∴ N₂F₄ produced = 0.0998 mol
converting moles to mass: m = nM = (0.0998)(14.01×2+19.00×4)
∴ N₂F₄ produced = 10.38 g
How much energy is involved when 100g of water is heated from 35°C to 115°C water vapor?
252,212 Joules of energy are required to heat 100g of water from 35°C to 115°C water vapor.
To calculate the amount of energy required to heat water from 35°C to 100°C, we use the specific heat capacity of water, which is 4.18 J/(g°C). This means that it takes 4.18 Joules of energy to heat one gram of water by one degree Celsius.
So, the energy required to heat 100 g of water from 35°C to 100°C can be calculated as follows:
Q1 = m × c × ΔT
Q1 = 100 g × 4.18 J/(g°C) × (100°C - 35°C)
Q1 = 26,212 Joules
Next, we need to calculate the amount of energy required to vaporize the water at 100°C. This is done using the heat of vaporization of water, which is 2260 J/g.
So, the energy required to vaporize 100 g of water at 100°C is:
Q2 = m × Lv
Q2 = 100 g × 2260 J/g
Q2 = 226,000 Joules
Therefore, the total energy required to heat 100 g of water from 35°C to 115°C water vapor is:
Q = Q1 + Q2
Q = 26,212 Joules + 226,000 Joules
Q = 252,212 Joules
Thus, 252,212 Joules of energy are required to heat 100g of water from 35°C to 115°C water vapor.
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Which sub atomic particles are similar in size
Answer:
Neutrons and Protons
Explanation:
Different elements can have subatomic particles of varying sizes. The size of an atom is defined by the size of its electron cloud, which is composed of electrons, and the size of its nucleus, which is composed of protons and neutrons. The atomic number and subsequently the identity of an element are determined by the number of protons in the nucleus. The quantity of protons and neutrons in the nucleus determines its size. The quantity of electrons in the electron cloud and the energy levels they are located at define its size. The size of atoms can differ depending on the element due to differences in the amount of protons, neutrons, and electrons.
The combustion of 136 g of methane (CH₄) in the presence of excess oxygen gas produces 353 g of carbon dioxide. [CH₄ + 2O₂ --> CO₂ + 2H₂O; C = 12.01 g/mol, H = 1.01 g/mol, O = 16.0 g/mol]
What is the percent yield?
a.)
0.385
b.)
0.026
c.)
0.947
d.)
0.00946
Taking into account definition of percent yield, the correct answer is option c): the percent yield for the reaction is 0.947.
Reaction stoichiometryIn first place, the balanced reaction is:
CH₄ + 2 O₂ → CO₂ + 2 H₂O
By reaction stoichiometry, the following amounts of moles of each compound participate in the reaction:
CH₄: 1 moleO₂: 2 molesCO₂: 1 moleH₂O: 2 molesThe molar mass of the compounds is:
CH₄: 16.05 g/moleO₂: 32 g/moleCO₂: 44.01 g/moleH₂O: 18.02 g/moleBy reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
CH₄: 1 mole ×16.05 g/mole= 16.05 gramsO₂: 2 moles ×32 g/mole= 64 gramsCO₂: 1 mole ×44.01 g/mole= 44.01 gramsH₂O: 2 moles×18.02 g/mole= 36.04 gramsMass of CO₂ formedThe following rule of three can be applied: if by reaction stoichiometry 16.05 grams of CH₄ form 44.01 grams of CO₂, 136 grams of CH₄ form how much mass of CO₂?
mass of CO₂= (136 grams of CH₄× 44.01 grams of CO₂)÷16.05 grams of CH₄
mass of CO₂= 372.92 grams
Then, 372.92 grams of CO₂ can be produced from 136 grams of CH₄.
Percent yieldThe percent yield is the ratio of the actual return to the theoretical return expressed as a percentage and this is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:
percent yield= (actual yield÷ theoretical yield)× 100%
where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product.
Percent yield for the reaction in this caseIn this case, you know:
actual yield= 353 gramstheorical yield= 372.92 gramsReplacing in the definition of percent yield:
percent yield= (353 grams÷ 372.92 grams)× 100%
Solving:
percent yield= 94.7%= 0.947
Finally, the percent yield for the reaction is 0.947.
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When a hydrogen atom is added to a polyatomic ion, the amount of negative charge . Following this pattern, we can see that hydrogen carbonate has a charge of and hydrogen sulfate has a charge of .
If we add one or two hydrogen ions to a polyatomic ion that has a 3-charge, as the phosphate ion (PO₄3-), it will still be a polyatomic ion. (Three H+ would entirely cancel out the 3-charge, turning it into a neutral molecule and removing it from the category of polyatomic ions.
Why does carbonate have a negative 2 charge?As a result, the carbonate ion has 2 more electrons than protons due to its negative charge. The doubly bonded oxygen in the carbonate ion is neutral, whereas each single bonded oxygen has a negative charge. This is the cause of the total charge of "-2," then.
An essential component of the atmosphere of stars like the Sun is the hydrogen anion.
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What does X represent for this transmutation? 9 4Be + 4₂He X+ ¹on ?
The result of the transformation, denoted by the symbol X, is 12 6C.
What does the radioactive decay symbol X stand for?The chemical symbol for the unstable nucleus, X, is represented by the nuclear equation, where the letter a stands for the particle's mass number and the letter b for the number of protons.
What is atom transmutation?the process of changing one chemical element into another. Since a transmutation involves a change to the atomic nuclei's structure, it can either be produced via a nuclear reaction (q.v. ), like neutron capture, or it can happen naturally due to radioactive decay, like alpha and beta decay (qq. v.).
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Calcium nitrate reacts with ammonium fluoride to make calcium fluoride and ammonium nitrate. When (4.479x10^1) mL of (4.61x10^-1) M calcium nitrate was added to (7.332x10^1) mL of (1.5835x10^0) M ammonium fluoride, 0.731 grams of calcium fluoride were isolated. How many moles of ammonium fluoride were initially added in this experiment (not necessarily reacted)?
The moles of ammonium fluoride initially added in this experiment was 0.0216 moles.
What is mole?Mole is a unit of measurement that is used in chemistry to measure the amount of a substance. It is a very important unit of measurement because it allows chemists to accurately measure the amount of a substance that is being used in a reaction. The mole is defined as the amount of a substance that contains the same number of particles as there are atoms in 12 grams of carbon-12..
First, we need to calculate the moles of calcium nitrate in the solution. We can do this by using the molarity and volume of the solution:
(4.61x10⁻¹ M)*(4.479x10¹ mL) = 0.0216 moles of calcium nitrate
(0.731 g)*(1 mol/55.847 g) = 0.0131 moles of calcium fluoride
(0.0216 moles)*(1 mol/1 mol)
= 0.0216 moles of ammonium fluoride
Therefore, the moles of ammonium fluoride initially added in this experiment was 0.0216 moles.
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5. An unknown metal has a mass of 4.67 g. It is heated to 95.1°C and then placed in a
calorimeter that contains 24.3 g of water at 21.7°C. The metal and water both reach
a final temperature of 24.6°C. What is the specific heat of this metal? What is the
unknown metal?
The unknown metal with C(metal) of 0.90J/gC and mass of 4.67g is aluminum.
CalorimeterThe metal's specific heat is calculated using the heat equation. It is important to note that the total heat (Q), which is the sum of the two heats (Qwater and Qmetal), is equal to zero at equilibrium.
Now, Q(total)=Q(water)+Q(metal)
0=m(water)
The specific heat of water, C(water), is equal to 4.18 J/g, while the other two components are water and metal.
The temperature of a metal is known as C(metal).
With the given values all substituted, we obtain 0=m(water) C(water)T(water) +m(metal).
CmetalΔTmetal=(24.3g)(4.184J/g°C) (24.6°C−21.7°C)+(4.67g) (Cmetal)(24.6°C−95.1°C)
The metal's specific heat is given by the equation C(metal)=0.90J/gC, which is simplified by placing C(metal) on one side of the equation.
Part (b):As a result, aluminum is the metal.
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The Ka value for ethanoic acid, CH3COOH is 1.79 x 10-5. What is the pH of an equimolar solution of ethanoic acid and Na+CH3COO-?
The pH of the solution can be calculated using the following steps:
Write the chemical equation for the dissociation of ethanoic acid:
CH3COOH + H2O ⇌ CH3COO- + H3O+
Write the equilibrium expression for the dissociation of ethanoic acid:
Ka = [CH3COO-][H3O+] / [CH3COOH]
Since the solution is equimolar in CH3COOH and CH3COO-, we can assume that the initial concentrations of CH3COOH and CH3COO- are equal. Let's use the variable x to represent the concentration of CH3COO- and CH3COOH in mol/L.
[CH3COOH] = x mol/L [CH3COO-] = x mol/L
Since CH3COOH is a weak acid, we can assume that only a small fraction of it dissociates in water. Let's use the variable y to represent the concentration of H3O+ ions in mol/L that are produced from the dissociation of CH3COOH. From the dissociation of ethanoic acid, we know that [CH3COO-] = [H3O+].
[CH3COO-] = y mol/L [H3O+] = y mol/L
Use the equilibrium expression to solve for the concentration of H3O+ ions:
Ka = [CH3COO-][H3O+] / [CH3COOH] 1.79 x 10^-5 = y^2 / x
Solving for y in terms of x, we get:
y = sqrt(Ka * x)
Calculate the pH of the solution using the equation:
pH = -log[H3O+]
pH = -log(y)
Substituting in the value of y from Step 5, we get:
pH = -log(sqrt(Ka * x))
Simplifying, we get:
pH = -0.5 * log(Ka * x)
Substituting in the value of Ka, we get:
pH = -0.5 * log(1.79 x 10^-5 * x)
Now we can calculate the pH for the solution by substituting the value of x as it is equimolar.
pH = -0.5 * log(1.79 x 10^-5 * x)
pH = -0.5 * log(1.79 x 10^-5 * 1)
pH = -0.5 * log(1.79 x 10^-5)
pH = 4.74
Therefore, the pH of an equimolar solution of ethanoic acid and Na+CH3COO- is 4.74.
Calculate the concentrations of all species in a 0.510 M NaCH3COO (sodium acetate) solution. The ionization constant for acetic acid is a=1.8×10−5.
[Na+]=
[OH−]=
[H3O+]=
[CH3COO−]=
[CH3COOH]=
The concentrations of all species in a 0.510 M NaCH₃COO (sodium acetate) solution: [Na+]= 0.510 M , [OH-]= 1.8x10⁻⁵ M , [H₃O+]= 1.8x10⁻⁵ M , [CH₃COO-]= 0.510 M and [CH₃COOH]= 0.510 - (1.8x10⁻⁵) = 0.50982 M.
What is concentration?Concentration is the ability to focus your attention on a single task or thought for a prolonged period of time. It involves being able to ignore distractions and to be able to work through any difficulties or obstacles that may arise. Concentration is an important skill to master in order to achieve success in any endeavor, whether it be academic, professional, or personal. Good concentration can help you to stay focused, organized, and productive. When you are able to concentrate, you can take in the information needed to make better decisions and solve problems. Concentration is a skill that can be developed with practice, such as by setting goals, breaking down tasks into smaller, manageable pieces, and avoiding distractions.
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