To solve this problem, we need to use Henry's Law, which states that the solubility of a gas in a liquid is directly 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 the Henry's Law constant (in mol/(L*atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.0019 mol/(L*atm),
P = 4.38 atm,
V = 1025 mL = 1.025 L (since 1 L = 1000 mL).

We can substitute these values into the formula to find C:

C = kP
C = 0.0019 mol/(L*atm) * 4.38 atm
C = 0.008322 mol/L

This is the concentration of NO in the water. To find the mass of NO that can be dissolved, we need to convert this concentration into grams. The molar mass of NO is approximately 30.01 g/mol, so:

mass = C * V * molar mass
mass = 0.008322 mol/L * 1.025 L * 30.01 g/mol
mass = 0.256 g

So, approximately 0.26 g of NO can be dissolved in 1025 mL of water at 25.0°C and a NO partial pressure of 4.38 atm.

Question

To solve this problem, we need to use Henry's Law, which states that the solubility of a gas in a liquid is directly 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 the Henry's Law constant (in mol/(L*atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.0019 mol/(L*atm),
P = 4.38 atm,
V = 1025 mL = 1.025 L (since 1 L = 1000 mL).

We can substitute these values into the formula to find C:

C = kP
C = 0.0019 mol/(L*atm) * 4.38 atm
C = 0.008322 mol/L

This is the concentration of NO in the water. To find the mass of NO that can be dissolved, we need to convert this concentration into grams. The molar mass of NO is approximately 30.01 g/mol, so:

mass = C * V * molar mass
mass = 0.008322 mol/L * 1.025 L * 30.01 g/mol
mass = 0.256 g

So, approximately 0.26 g of NO can be dissolved in 1025 mL of water at 25.0°C and a NO partial pressure of 4.38 atm.

Knowee AI · Accepted Answer

To solve this problem, we need to use Henry's Law, which states that the solubility of a gas in a liquid is directly 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 the Henry's Law constant (in mol/(L*atm)),
P is the partial pressure of the gas (in atm).

Given:
k = 0.0019 mol/(L*atm),
P = 4.38 atm,
V = 1025 mL = 1.025 L (since 1 L = 1000 mL).

We can substitute these values into the formula to find C:

C = kP
C = 0.0019 mol/(L*atm) * 4.38 atm
C = 0.008322 mol/L

This is the concentration of NO in the water. To find the mass of NO that can be dissolved, we need to convert this concentration into grams. The molar mass of NO is approximately 30.01 g/mol, so:

mass = C * V * molar mass
mass = 0.008322 mol/L * 1.025 L * 30.01 g/mol
mass = 0.256 g

So, approximately 0.26 g of NO can be dissolved in 1025 mL of water at 25.0°C and a NO partial pressure of 4.38 atm.

At 25.0°C the Henry's Law constant for nitrogen monoxide NO gas in water is /0.0019Matm.Calculate the mass in grams of NO gas that can be dissolved in 1025.mL of water at 25.0°C and a NO partial pressure of 4.38atm.Round your answer to 2 significant digits.

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