The concentration of CO2 in water at 20°C is 1.00×10-5 M. The Henry’s constant for CO2 dissolution in water is 3.91×10-2 M atm-1 at 20°C. What is the partial pressure of CO2 in the air?
Question
The concentration of CO2 in water at 20°C is 1.00×10-5 M. The Henry’s constant for CO2 dissolution in water is 3.91×10-2 M atm-1 at 20°C. What is the partial pressure of CO2 in the air?
Solution
To find the partial pressure of CO2 in the air, we can use Henry's Law, which states that the concentration of a gas in a liquid is proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is:
P = C / K
where: P is the partial pressure of the gas, C is the concentration of the gas, and K is Henry's constant.
Given: C = 1.00×10^-5 M (concentration of CO2 in water) K = 3.91×10^-2 M atm^-1 (Henry's constant for CO2 dissolution in water)
Substitute these values into the formula:
P = (1.00×10^-5 M) / (3.91×10^-2 M atm^-1)
Solving this gives:
P = 2.56 x 10^-4 atm
So, the partial pressure of CO2 in the air is 2.56 x 10^-4 atm.
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