how long will one iv bag last for the following medication order? potassium chloride 10 meq in d5w 50 ml iv q 24h rate: 50 ml/hr

The limiting reagent is sebacoyl chloride because we have fewer moles of it than 1,6-diamino hexane.

The reaction between 1,6-diamino hexane and sebacoyl chloride forms nylon-6,10, and the balanced chemical equation for the reaction is:

1,6-diaminohexane + sebacoyl chloride → nylon-6,10 + 2 HCl

To determine the limiting reagent, we need to compare the moles of each reactant to the stoichiometric ratio in the balanced equation.

Let's assume we have 2.00 moles of 1,6-diaminohexane and 1.50 moles of sebacoyl chloride.

The stoichiometric ratio in the balanced equation is 1:1, so we need an equal number of moles of both reactants to form nylon-6,10.

From the given amounts, we can calculate the moles of each reactant:

moles of 1,6-diaminohexane = 2.00 moles

moles of sebacoyl chloride = 1.50 moles

Since the stoichiometric ratio is 1:1, the limiting reagent is sebacoyl chloride because we have fewer moles of it than 1,6-diaminohexane.

To calculate the percent yield of nylon, we need to know the mass of the product formed. We can use the molecular weight of one repeating monomer unit of nylon-6,10 to calculate the weight of the product.

The molecular weight of one repeating monomer unit of nylon-6,10 is:

molecular weight of 1,6-diaminohexane: 116.20 g/mol

molecular weight of sebacoyl chloride: 260.41 g/mol

molecular weight of one repeating monomer unit: 226.61 g/mol (116.20 + 260.41 - 2*36.46)

To calculate the theoretical yield of nylon, we need to use the stoichiometric ratio and the amount of limiting reagent. Since the limiting reagent is sebacoyl chloride, we will use its moles to calculate the theoretical yield of nylon:

moles of sebacoyl chloride = 1.50 moles

moles of nylon-6,10 = 1.50 moles (from stoichiometric ratio)

The mass of the theoretical yield of nylon-6,10 is:

mass of nylon-6,10 = moles of nylon-6,10 x molecular weight of nylon-6,10

mass of nylon-6,10 = 1.50 moles x 226.61 g/mol = 339.92 g

Assuming that the actual yield of nylon-6,10 is 280.00 g, the percent yield is:

percent yield = (actual yield / theoretical yield) x 100%

percent yield = (280.00 g / 339.92 g) x 100%

percent yield = 82.36%

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Complete question:

what is the limiting reagent in the reaction between 1,6-diaminohexane and sebacoyl chloride. calculate the percent yield of nylon using molecular weight of one repeating monomer unit for the weight of the product

actual yield for nylon : 280.00 g

According to the second law of Faraday, the oxidation number of gold ions is +3.

The second law of Faraday is also known as Faraday's law of electrolysis. According to this, the quantity of a substance that is deposited or released during electrolysis is directly proportional to the amount of electric charge that is transported through the electrolyte.

Given information,

Mass of silver (Ag) deposited = 0.732 g

Mass of gold (Au) deposited = 0.446 g

According to this law,

Weight of Ag/Equivalent weight of Ag = Weight of Au/Equivalent weight of Au

0.732/108 = 0.446/196.96 × valency

Since the equivalent weight of Ag is 108g and the equivalent weight of Au is 196.96g.

0.0067 = 0.0022  × valency

Valency = 0.0067/ 0.0022

Valency = 3

Therefore, the oxidation state of the gold ion (Au⁺³) is +3.

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One molecule of this substance has the molecular formula CH₂ClO, which is methoxychloro. to ascertain how many oxygen atoms there are in 2 molecules of methoxychloro.

To create dioxygen, or oxygen, two oxygen atoms must make a covalent double bond with one another. Typically, oxygen exists as a molecule. It has the name dioxygen.

With an electrical configuration of (2, 6) and an atomic number of 8, oxygen lacks two more electrons to complete an octet. By exchanging two pairs of electrons with another oxygen atom, the oxygen atom becomes stable. A diatomic oxygen molecule is one that contains two oxygen atoms.

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using many methods I gess I am not good at drawing

Answer: Different isotopes of the same sample have different scattering signals in neutron experiments due to their varying neutron cross-sections.

The term neutron scattering refers to a type of scattering in which neutrons collide with a target material, resulting in the emission of secondary particles. Because the neutron is a subatomic particle, it cannot be directly detected.

The effect of its presence, however, can be seen in the pattern of scattered secondary particles. Neutrons are scattered in much the same way that light is, except that they are much less affected by surface roughness and other surface-related issues.

This implies that neutron scattering is a more efficient tool for investigating material microstructures than other kinds of scattering. Neutron scattering's biggest advantage is its sensitivity to the atomic nuclei of a sample's constituent atoms.

Neutrons, unlike other subatomic particles, have no electric charge, making them less likely to be deflected by the electrons surrounding atomic nuclei, and more likely to penetrate deep into a sample's interior.

As a result, neutron scattering may reveal information about the locations and movements of atomic nuclei in materials that is inaccessible to other methods. Cross-sections of neutron scattering: The cross-section of a neutron scattering material is the probability of a neutron scattering off that material.

In other words, it's the ratio of the number of neutrons scattered per second per unit area of material to the number of neutrons striking the material per second per unit area.

Because the probability of a neutron scattering off a given isotope varies based on the neutron's energy and the isotopes present, the cross-section of a sample's individual isotopes influences the total neutron scattering signal produced by the sample.

Different isotopes of the same sample have different scattering signals in neutron experiments due to their varying neutron cross-sections.

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The enthalpy change when 100. g of ice at 0.0°C is heated to liquid water at 50.0°C is equal to 333J/g x 100g = 33300 J.

This is because the heat of fusion of water is 333J/g and it takes 33300J of energy to melt 100g of ice at 0.0°C.

The process of melting the ice can be broken down into two steps. First, the ice needs to be heated from 0.0°C to its melting point (0.0°C).

This requires energy to overcome the intermolecular forces that are keeping the ice solid, but no heat is absorbed or released. Second, the ice needs to be heated from its melting point to 50.0°C.

This is when the heat of fusion is released and 333J of energy is absorbed for every gram of ice melted. Therefore, 333J/g x 100g = 33300J of energy must be supplied to the system for the ice to melt and reach 50.0°C.

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Certain reaction has an activation energy of 34.34 kj/mol. At  428.0 kelvin temperature will the reaction proceed 3.00 3.00 times faster than it did at 357 k?

The physical concept of temperature indicates in numerical form how hot or cold something is. A thermometer is used to determine temperature. Thermometers are calibrated using a variety of temperature scales, which historically defined distinct reference points and thermometric substances. The most popular scales are the Celsius scale, sometimes known as centigrade, with the unit symbol °C, the Fahrenheit scale (°F), and the Kelvin scale (K), with the latter being mostly used for scientific purposes. One of the International System of Units' (SI) seven base units is the kelvin.

k1/k2 = [tex]e^{((Ea/R) * ((1/T2) - (1/T1)}[/tex]

Ea = 34.34 kJ/mol × 1000 J/kJ

    = 34,340 J/mol

3.00 = [tex]e^{((34,340 J/mol / (8.314 J/mol K)) × ((1/T2) - (1/357 K)))}[/tex]

ln(3.00) = (34,340 J/mol / (8.314 J/mol K))×((1/T2) - (1/357 K))

T2 = 1 / (ln(3.00) / (34,340 J/mol / (8.314 J/mol K)) + (1/357 K)) = 428.0 K

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The volume in liters of a 0.020mm barium chlorate solution that contains 375 mmol of barium chlorate is 18.75 L.

To calculate the volume of barium chlorate in liters, we can use the formula of concentration. The formula of concentration is

C = n/V

where

C = Concentration

n = moles of the solute

V = volume of the solution

To calculate the volume of the solution in liters, we need to first calculate the moles of the solute ([tex]BaCl_{2}[/tex]). We are given moles of [tex]BaCl_{2}[/tex] = 375 mmol

Now, n = 375 mmol. So, by using the formula of concentration:

C = n/VC = 0.020 mm

V = n/CV

= 375 mmol/0.020 mmV

= 18750 mL

We know that 1 L = 1000 mL. So, the volume of the solution in liters

= 18750/1000L

= 18.75 L

Thus, the volume of the solution in liters is 18.75 L.

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In a cyclic voltammogram of an irreversible electrochemical reaction, only one peak is present (either anodic or cathodic) due to the limited reversibility of the reaction.

An irreversible reaction cannot be completely reversed so when the potential of the reaction is increased, the reaction will proceed in the same direction, leading to the formation of a single peak.

The peak represents the forward reaction, either the oxidation or reduction of the species in the reaction.

The magnitude of the peak depends on the rate of the forward reaction and the degree of reversibility of the reaction.

When the potential of the reaction is increased, the reaction will move further in the same direction, and the peak will become more prominent.

The peak will reach a maximum size when the reaction reaches its equilibrium potential, which occurs when the rate of the forward and reverse reactions are equal.

The magnitude of the peak also depends on the rate of diffusion of the species in the reaction. The peak will be smaller when the rate of diffusion is slow, and it will be larger when the rate of diffusion is fast.

The shape of the peak will depend on the degree of reversibility of the reaction, with more symmetrical peaks for reversible reactions and more asymmetrical peaks for irreversible reactions.

Only one peak is present in a cyclic voltammogram of an irreversible electrochemical reaction due to the limited reversibility of the reaction.

The magnitude of the peak is determined by the rate of the forward reaction, the rate of diffusion of the species, and the degree of reversibility of the reaction.

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If we assume that the melting points and TLC are in agreement, then we can use them to determine the purity of the solids.

The purest solid would have the highest melting point and the most distinct TLC spot. We can compare the values to ascertain which solid is the purest if the melting points and TLC are in agreement. It may be a sign that the extraction was unsuccessful or that there were impurities in the sample if there is a significant difference between the melting points or the spots on the TLC.

It's crucial to remember that melting points and TLC are not always accurate indications of purity because other variables can influence them. However, they can be a helpful tool for determining the success of an extraction experiment if the values are consistent and in agreement.

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The substance with a pH that is lower than bleach but higher than egg whites would have a pH between 8 and 12.

pH is a measure of the acidity or basicity (alkalinity) of a solution. It is measured on a scale from 0 to 14, with a pH of 7 considered neutral. pH values below 7 indicate acidity, while pH values above 7 indicate basicity.

Household bleach has a pH of around 12-13, while egg whites have a pH of around 7-8. Therefore, the substance with a pH that is lower than bleach but higher than egg whites would have a pH between 8 and 12.

Substances with a pH in this range include baking soda (pH around 9), milk of magnesia (pH around 10), and ammonia solution (pH around 11). However, without further information, it is impossible to determine the exact substance with certainty.

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4.83 x 10^24 atoms are there in 32.10 g of He.

To determine the number of atoms in 32.10 g of He, we first need to convert the mass to moles using the atomic mass of He, which is 4.003 g/mol.

number of moles of He = 32.10 g / 4.003 g/mol = 8.024 mol He

Next, we use Avogadro's number, which is 6.022 x 10^23 atoms/mol, to calculate the number of atoms in 8.024 mol of He:

8.024 mol He x 6.022 x 10^23 atoms/mol = 4.83 x 10^24 atoms

Therefore, there are approximately 4.83 x 10^24 atoms in 32.10 g of He.

Atoms are the fundamental matter units that comprise everything around us, from the air we breathe to the food we consume. They are made up of three different sorts of particles: protons, neutrons, and electrons.

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It appears that you are attempting to identify the various elements of each of these tests shown in the scenarios for this topic.

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Answer:

Ra3P2

Explanation:

Ra is +2

P is -3

Ra3P2

The activation energy for a forward reaction is not the same as the activation energy for the reverse of the same reaction. It is because of the reason that activation energy is the energy needed for a reaction to occur.

The energy barrier for a forward reaction is distinct from the energy barrier for a backward reaction. The energy required to break bonds in the reactants is known as activation energy.

Only those molecules with sufficient kinetic energy can overcome the activation energy barrier and form new products. The energy that must be overcome in order to transform reactants into products is referred to as activation energy. If the activation energy for a reaction is lower, the reaction will proceed more quickly than if it were higher.

The activation energy of a forward reaction is not the same as the activation energy of a reverse reaction since the energy requirements for each reaction are unique.

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Lithium carbonate contains 18.78% mass percent lithium. It should be noted that a compound's overall percentage composition of all its constituent elements is always 100%.

Only depression related to bipolar illness is authorized for lithium use. When combined with an antidepressant, it may also be successful in alleviating other types of depression, although further research is required. Discuss the possibility of adding lithium with your doctor if you are on an antidepressant but are still experiencing symptoms.

This substance is employed for the treatment of mania and depression (bipolar disorder). By bringing certain natural compounds back into equilibrium in the brain, it helps to calm mood and lessen excessive behavior.

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Answer:

To convert molecules of C2H2 to grams, we need to use the molar mass of C2H2, which is 26.04 g/mol.

First, we need to calculate the number of moles in 7.41 x 10^24 molecules of C2H2:

7.41 x 10^24 molecules / 6.022 x 10^23 molecules/mol = 12.31 mol

Then, we can use the formula:

mass = moles x molar mass

mass = 12.31 mol x 26.04 g/mol = 320.4624 g

Therefore, 7.41 x 10^24 molecules of C2H2 is equivalent to 320.4624 grams.

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Metallic bonds a. allow for high electrical conductivity in a material. Metallic bonds are non-directional. They also allow a material to plastically deform.

Metallic bonding is the bonding between the positively charged nuclei of metal atoms and the electrons in the metal's outermost electron shell. Metallic bonding in metals is believed to be like a sea of electrons that are free to move throughout the entire metallic crystal. This is why metals conduct heat and electricity so effectively, making them excellent conductors.

The atoms in a metal are not held together by covalent bonds, but rather by metallic bonds. They are typically held together in a crystal lattice. The electrons in metals are not held to any specific atom or molecule, but rather they move around freely among the metal atoms' positively charged ion cores. The metallic bond is a non-directional bond. The electrons in the metal are delocalized, which means they are free to move around the metal lattice.

As a result, metals are malleable and ductile, meaning they can be formed into sheets or drawn into wires. Metals can also be deformed without being broken or shattered because the metallic bond is non-directional. In general, metals are good conductors of electricity and heat because their free electrons can easily move in response to an electric or thermal current. So, the correct option are: metallic bonds allow for high electrical conductivity in a material, metallic bonds are non-directional, and metallic bonds allow a material to plastically deform.

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Answer:

2.41 m

Explanation:

2.41×10×10=241cm

241÷100=2.41

Magnesium carbonate breaks down into solid magnesium (MgO) & gaseous carbon dioxide in the aforementioned mechanism, which is a chemical property (CO2).

In these equations, chemical reactions are represented by chemical formulae and symbols. Chemical equations have two sides: the reactants are on the left, and the products are on the right.

Chemical equations represent the transformation of reactants into products in this process. Take the combination of iron (Fe) with sulfur (S) to create iron sulfide as an example. Fe(s) = S(s) + FeS (s) Iron and sulfur react, as indicated by the plus symbol.

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The reaction between Na2S and CuSO4 goes to completion, meaning that all of the available reactants will react. Therefore, the amount of excess reactant remaining is 0 g.

To calculate the amount of each reactant remaining, we need to look at the stoichiometric coefficients of the reaction. Na2S has a coefficient of 1, while CuSO4 has a coefficient of 2. This means that for every 1 mole of Na2S, 2 moles of CuSO4 are needed. We can use the given masses of each reactant to calculate the moles present.

For Na2S: 15.5 g x (1 mol/142 g) = 0.109 mol

For CuSO4: 12.1 g x (1 mol/159 g) = 0.076 mol

Since Na2S has a coefficient of 1, 0.109 mol is the amount of Na2S remaining. However, for CuSO4 the coefficient is 2, so we need to divide 0.076 mol by 2 to get the amount of CuSO4 remaining: 0.038 mol.

Finally, we can convert back to grams to get the amount of each reactant remaining:

Na2S: 0.109 mol x (142 g/1 mol) = 15.3 g

CuSO4: 0.038 mol x (159 g/1 mol) = 6.1 g

Therefore, the amount of excess reactant remaining is 0 g, and the amount of each reactant remaining is 15.3 g of Na2S and 6.1 g of CuSO4.

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The empirical formula of the compound that produces 330 g of carbon, 69.5 g of hydrogen, and 440.4 g of oxygen upon decomposition is CHO2.

The empirical formula of a compound is the simplest whole-number ratio of atoms present in it. Follow the below steps to calculate the empirical formula of the given compound: Calculate the mass of each element present in the compound.

Calculate the mole of each element present in the compound by dividing its mass by its atomic mass. Determine the mole ratio by dividing each mole value by the smallest mole value obtained. Rearrange the ratio obtained in step 3 in the form of whole numbers. Moles of hydrogen/moles of oxygen = 69.5/27.5 = 2.53 ≈ 2.5Moles of oxygen/moles of oxygen = 27.5/27.5 = 1Therefore, the mole ratio of carbon: hydrogen: oxygen = 1: 2.5: 1Rearranging the above ratio to whole numbers, we get the mole ratio of carbon: hydrogen: oxygen as 2: 5: 2. The empirical formula of the compound is therefore CHO2.

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The reaction has reached its equivalence point once it is complete.

To determine if the reaction has reached its equivalence point once the reaction is complete, we must first calculate the moles of each compound:

HCl moles = 1.0 M x (10.0 mL / 1000 mL/L) = 0.01 mol

NaOH moles = 2.0 M x (5.0 mL / 1000 mL/L) = 0.01 mol

The two compounds react in a 1:1 ratio.

There are now no more moles of HCl or NaOH left to react since they have equal moles.

We can thus conclude that the reaction has reached its equivalence point as soon as the reaction is over. Since the moles of both HCl and NaOH have been completely neutralized, the pH at the equivalence point is 7.

This indicates that the reaction has reached its equivalence point once it has finished.

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The solution that has the highest vapor pressure is the one with the lowest boiling point. The lower the boiling point, the higher the vapor pressure.

Vapor pressure is the pressure exerted by the vapor of a substance in equilibrium with its liquid or solid phase. When the rate of evaporation and the rate of condensation is equal, equilibrium occurs. At a particular temperature, each liquid has a distinct vapor pressure that is directly proportional to its temperature. A liquid with a low boiling point has a higher vapor pressure than one with a high boiling point.

The glucose and sucrose solutions are both nonvolatile solutes, whereas potassium acetate is a volatile solute. As a result, the potassium acetate solution has a higher vapor pressure than either the glucose or sucrose solutions. The answer is option C.10.0 g of potassium acetate in 100.0 ml of water.

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The combination of elements that are required for a compound to be considered organic are carbon and hydrogen. The correct answer among the given options is carbon and hydrogen.

Organic compounds are the fundamental components of life and are classified by the presence of carbon atoms, which are covalently linked to one another and to other elements such as oxygen, nitrogen, and sulfur, as well as by the lack of ionic bonding.

To summarize, an organic compound is a compound that contains carbon atoms bonded to hydrogen atoms, among other elements, in a covalent bond. The majority of organic compounds contain a carbon-carbon bond, which is the foundation of organic chemistry.

The following are some examples of organic compounds:

Methane, CH4

Ethanol, C2H5OH

Ethanoic acid, CH3COOH

Acetone, (CH3)2CO

Amino acid glycine, NH2CH2COOH

As a result, the correct combination of elements that are required for a compound to be considered organic are carbon and hydrogen.

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Answer:
To calculate the number of atoms of H and C in 0.160 mol of C6H14O, we need to first determine the number of moles of each element present in C6H14O.

The molecular formula of C6H14O shows that there are 6 carbon atoms, 14 hydrogen atoms, and 1 oxygen atom in each molecule of C6H14O.

The molar mass of C6H14O can be calculated as:

Molar mass of C6H14O = (6 × atomic mass of C) + (14 × atomic mass of H) + (1 × atomic mass of O)

= (6 × 12.01 g/mol) + (14 × 1.01 g/mol) + (1 × 16.00 g/mol)

= 86.18 g/mol

Therefore, 0.160 mol of C6H14O has a mass of:

Mass = molar mass × number of moles

= 86.18 g/mol × 0.160 mol

= 13.79 g

Now we can calculate the number of atoms of H and C in 0.160 mol of C6H14O.

Number of atoms of H:

Number of moles of H = 14 × 0.160 mol = 2.24 mol

Number of atoms of H = 2.24 mol × Avogadro's number

= 2.24 mol × 6.022 × 10^23/mol

= 1.35 × 10^24 atoms of H

Therefore, there are 1.35 × 10^24 atoms of hydrogen in 0.160 mol of C6H14O.

Number of atoms of C:

Number of moles of C = 6 × 0.160 mol = 0.96 mol

Number of atoms of C = 0.96 mol × Avogadro's number

= 0.96 mol × 6.022 × 10^23/mol

= 5.78 × 10^23 atoms of C

Therefore, there are 5.78 × 10^23 atoms of carbon in 0.160 mol of C6H14O.

Explanation:

(+61.3) is the specific rotation of pure (s)-carvone if a sample of (r)-carvone of 85% ee has a specific rotation of -52.

A chiral chemical compound's unique rotation is a characteristic in chemistry. It is described as the shift in monochromatic plane-polarized light's orientation, expressed as the product of distance and concentration, as the light passes through a sample of a substance dissolved in solution. Dextrorotary substances are those that spin a plane polarised light beam's polarisation plane clockwise, and they correlate to positive specific rotation values.

[α] = α / (c×l)

[α] =specific rotation

α = observed rotation

c=concentration in g/mL

l =path length in dm

[α] = (-52)/(1×1)

    = -52

(-52) = (0.85)×αr + (0.15)×αs

αs= (-52 - 0.85×αr) / 0.15

[α] = αs

    = (-52 - 0.85αr) / 0.15

(-52) = (0.85)(+112.0) + (0.15)α

α = (+61.3)

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The volume of oxygen gas will it occupy when the pressure is changed to 912 torr and temperature remains constant is 2.41 L.

PV = nRT is the equation for an ideal gas. In this equation, P stands for the ideal gas's pressure, V for the ideal gas' volume, n for the total amount of the ideal gas expressed in moles, R for the universal gas constant, and T for temperature.

a formula that converts the volume and pressure of a mole of gas into its combined thermodynamic temperature and gas constant. At low pressures, the equation is a decent approximation for actual gases and is precise for an ideal gas. Also known as the ideal gas law and ideal gas equation.

According to ideal gas equation

PV = nRT

Here P is pressure, V is Volume, n is mole, R is gas constant, T is temperature

Now if T is constant the nRT term will become constant

So PV = constant

And P1V1 = P2V2

now P1 = 1156 torr        V1 = 1.9L

        P2 = 912 torr          V2 = ??

Put all values

1156 × 1.9 = 912 × V2

V2 = 2.41 L.

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The mass of [tex]Ag_2SO_4[/tex] precipitates out is 3.8975 g

We need to use the stoichiometry of the chemical reaction between [tex]AgNO_3[/tex] and [tex]Na_2SO_4[/tex] to determine how much [tex]Ag_2SO_4[/tex] will be formed. The balanced chemical equation for the reaction is:

[tex]AgNO_3 + Na_2SO_4[/tex] → [tex]Ag_2SO_4 + 2NaNO_3[/tex]

Moles of [tex]AgNO_3[/tex] = volume (in L) × molarity

                            = 0.025 L × 0.500 mol/L

                            = 0.0125 mol

Moles of [tex]Na_2SO_4[/tex] = volume (in L) × molarity

                             = 0.040 L × 0.250 mol/L

                             = 0.010 mol

The number of moles of [tex]Ag_2SO_4[/tex] formed is equal to the number of moles of [tex]AgNO_3[/tex]:

Moles of Silver nitrate ([tex]Ag_2SO_4[/tex]) = 0.0125 mol

Calculate the mass of [tex]Ag_2SO_4[/tex]:

Mass of [tex]Ag_2SO_4[/tex]= moles of [tex]Ag_2SO_4[/tex] × molar mass

Mass of [tex]Ag_2SO_4[/tex] = 0.0125 mol × 311.8 g/mol

Mass of [tex]Ag_2SO_4[/tex] = 3.8975 g

Therefore, the mass of [tex]Ag_2SO_4[/tex] formed is 3.8975 g.

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The property that affects a substance's saturation temperature is Pressure.

Saturation temperature is the temperature at which a liquid and a gas have the same vapor pressure. The vapor pressure of a liquid is affected by temperature, and at the saturation temperature, the vapor pressure of the liquid equals the pressure of the surrounding atmosphere.

A substance's saturation temperature is influenced by several variables. Pressure is one of the variables that influences the saturation temperature of a substance. When the pressure surrounding a substance rises, its saturation temperature rises.

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