# How Many Moles of CO Dissolve in Water According to Henry's Law?

• Chemistry
• imxaxpunk
Your Name] In summary, we can use the Henry's law equation to find the solubility of CO in water at a given temperature and partial pressure. We can also use it to calculate the partial pressure needed to maintain a certain concentration of CO2 in a solution. Using this equation, we found that for a partial pressure of 2.75 atm, 2.67 * 10^-3 moles of CO will dissolve in 1.00 L of water. For the second question, a pressure of 3.5 atm is needed to maintain a concentration of 0.12 M in club soda at 25 degrees C.
imxaxpunk

## Homework Statement

The henry's law constant (k) for carbon monoxide in water at 25 degree C is 9.71 * 10 ^-4 mol/(L*atm)

How many moles of CO will dissolve in 1.00 L of water if the partial pressure of CO is 2.75 atm?

## Homework Equations

waht pressure of carbon dioxide is required to keep the carbon dioxide concentration in a bottle of club soda at .12 M at 25 degrees C?
Info: Kh for Co2 at 25 degrees C = 3.4 * 10^-2 M/atm

Answer to that is 3.5 atm

## The Attempt at a Solution

s(g) = Kh * Pg
Since i don't have the Molarity i have no idea what to do.
M = moles solute ( i don't know if the water or CO is the solvent or solute)
divided by L solution

(9.71*10^-4mol/L*atm)(2.75 atm) = 2.67 *10^-3 mol/L
2.67*10^-3 mol/L * 1.00 L = 2.67*10^-3 mol
i have no idea what to do from there

To find the number of moles of CO that will dissolve in 1.00 L of water, we can use the Henry's law equation:
s(g) = k * Pg
where s(g) is the solubility of CO in water, k is the Henry's law constant, and Pg is the partial pressure of CO.
In this case, we have:
s(g) = (9.71 * 10^-4 mol/(L*atm)) * (2.75 atm) = 2.67 * 10^-3 mol/L
This means that 2.67 * 10^-3 moles of CO will dissolve in 1.00 L of water.
As for your second question about the pressure of carbon dioxide needed to maintain a concentration of 0.12 M in club soda, we can use a similar equation:
s(g) = k * Pg
where s(g) is the solubility of CO2 in water, k is the Henry's law constant, and Pg is the partial pressure of CO2.
We can rearrange this equation to solve for Pg:
Pg = s(g)/k
Plugging in the given values, we have:
Pg = (0.12 M)/(3.4 * 10^-2 M/atm) = 3.5 atm
Therefore, a pressure of 3.5 atm of CO2 is needed to maintain a concentration of 0.12 M in club soda at 25 degrees C.
I hope this helps!

## 1. What is Henry's law?

Henry's law is a gas law that describes the relationship between the concentration of a gas in a liquid and the partial pressure of that gas above the liquid.

## 2. How is Henry's law used in finding moles?

Henry's law can be used to find the number of moles of a gas in a liquid by multiplying the concentration of the gas by the volume of the liquid. This can be represented by the equation C = kP, where C is the concentration, k is the Henry's law constant, and P is the partial pressure of the gas.

## 3. What is the Henry's law constant?

The Henry's law constant is a proportionality constant that relates the concentration of a gas in a liquid to its partial pressure. It is unique for each gas and is dependent on factors such as temperature and the properties of the liquid.

## 4. How does temperature affect Henry's law?

According to Henry's law, the solubility of a gas in a liquid decreases with increasing temperature. This means that as the temperature increases, the concentration of the gas in the liquid decreases.

## 5. What are some real-world applications of Henry's law?

Henry's law has many practical applications, such as in the carbonation of beverages, where the solubility of carbon dioxide in water is key. It is also important in understanding gas exchange in the human body, as well as in environmental processes such as the release of gases from bodies of water. Additionally, Henry's law is used in industries such as chemical manufacturing and wastewater treatment.

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