To solve this problem, we need to use Henry's Law, which states that the amount of gas that dissolves in a liquid at a given temperature is proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is:

C = kP

where:
C is the concentration of the gas in the liquid (in mol/L),
k is Henry's Law constant (in mol/(L.atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.025 mol/(L.atm),
P = 3.52 atm,
V = 925 mL = 0.925 L (since 1 L = 1000 mL).

We need to find C, the concentration of N2O in the water.

Step 1: Substitute the given values into the Henry's Law formula:

C = kP
C = 0.025 mol/(L.atm) * 3.52 atm
C = 0.088 mol/L

This is the concentration of N2O in the water.

Step 2: To find the mass of N2O that can be dissolved in 925 mL of water, we need to convert the concentration (in mol/L) to mass (in g). We do this by multiplying the concentration by the volume of the water and the molar mass of N2O (44.01 g/mol):

mass = C * V * molar mass
mass = 0.088 mol/L * 0.925 L * 44.01 g/mol
mass = 3.6 g

So, 3.6 g of N2O gas can be dissolved in 925 mL of water at 25.0°C and a N2O partial pressure of 3.52 atm. Rounded to 2 significant digits, the answer is 3.6 g.

Question

To solve this problem, we need to use Henry's Law, which states that the amount of gas that dissolves in a liquid at a given temperature is proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is:

C = kP

where:
C is the concentration of the gas in the liquid (in mol/L),
k is Henry's Law constant (in mol/(L.atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.025 mol/(L.atm),
P = 3.52 atm,
V = 925 mL = 0.925 L (since 1 L = 1000 mL).

We need to find C, the concentration of N2O in the water.

Step 1: Substitute the given values into the Henry's Law formula:

C = kP
C = 0.025 mol/(L.atm) * 3.52 atm
C = 0.088 mol/L

This is the concentration of N2O in the water.

Step 2: To find the mass of N2O that can be dissolved in 925 mL of water, we need to convert the concentration (in mol/L) to mass (in g). We do this by multiplying the concentration by the volume of the water and the molar mass of N2O (44.01 g/mol):

mass = C * V * molar mass
mass = 0.088 mol/L * 0.925 L * 44.01 g/mol
mass = 3.6 g

So, 3.6 g of N2O gas can be dissolved in 925 mL of water at 25.0°C and a N2O partial pressure of 3.52 atm. Rounded to 2 significant digits, the answer is 3.6 g.

Knowee AI · Accepted Answer

To solve this problem, we need to use Henry's Law, which states that the amount of gas that dissolves in a liquid at a given temperature is proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is:

C = kP

where:
C is the concentration of the gas in the liquid (in mol/L),
k is Henry's Law constant (in mol/(L.atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.025 mol/(L.atm),
P = 3.52 atm,
V = 925 mL = 0.925 L (since 1 L = 1000 mL).

We need to find C, the concentration of N2O in the water.

Step 1: Substitute the given values into the Henry's Law formula:

C = kP
C = 0.025 mol/(L.atm) * 3.52 atm
C = 0.088 mol/L

This is the concentration of N2O in the water.

Step 2: To find the mass of N2O that can be dissolved in 925 mL of water, we need to convert the concentration (in mol/L) to mass (in g). We do this by multiplying the concentration by the volume of the water and the molar mass of N2O (44.01 g/mol):

mass = C * V * molar mass
mass = 0.088 mol/L * 0.925 L * 44.01 g/mol
mass = 3.6 g

So, 3.6 g of N2O gas can be dissolved in 925 mL of water at 25.0°C and a N2O partial pressure of 3.52 atm. Rounded to 2 significant digits, the answer is 3.6 g.

At 25.0°C the Henry's Law constant for dinitrogen monoxide N2O gas in water is /0.025Matm.Calculate the mass in grams of N2O gas that can be dissolved in 925.mL of water at 25.0°C and a N2O partial pressure of 3.52atm.Round your answer to 2 significant digits.

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