A vessel of 9.49 L in volume contains 3.37 L of pure water at 25¡ÆC. A partial pressure of 4.73 atm of CO2 is quickly injected into the space above the water. Calculate the partial pressure of carbon dioxide remaining once the solution has become saturated with the gas. Henry's constant for CO2 at this temperature is 0.0350 M atm-1.

Thanks

To find the partial pressure of carbon dioxide remaining once the solution has become saturated, we can use Henry's Law.

Henry's Law states that the partial pressure of a gas above a liquid is directly proportional to the concentration of that gas in the liquid at a given temperature. The equation representing Henry's Law is:

P = k * C,

where P is the partial pressure of the gas, k is Henry's constant, and C is the concentration of the gas in the liquid.

First, we need to calculate the concentration of carbon dioxide in the water. We know the volume of water (3.37 L) and that it is pure, so the concentration of carbon dioxide in the water is 0 M (since there is no CO2 initially present in the water).

Next, we can find the initial partial pressure of CO2. This is the partial pressure immediately after the CO2 is injected into the space above the water. The initial partial pressure of CO2 is given as 4.73 atm.

Since the solution becomes saturated with CO2, the final partial pressure of CO2 will be the same as the calculated partial pressure based on Henry's Law.

Using the equation P = k * C, we can rearrange it to solve for P:

P = k * C
P = k * 0
P = 0

This means that the final partial pressure of CO2 will be 0 atm, since all of the CO2 injected into the space above the water will dissolve in the water until it reaches saturation.