Question

How many moles of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at ${25}^{\circ }C$?
Given: $K_H$ of $C{O}_2$ in water = 29.76 atm/(mol/L) at ${25}^{\circ }C$

• A. 0.02
• B. 0.06
• C. 0.04
• D. 0.08

Answer 1

The correct option is D 0.08

When a gas is dissolved in a liquid, the concentrations will eventually reach equilibrium between the source of the gas and the solution. Henry's Law shows the concentration of a solute gas in a solution is directly proportional to thepartial pressureof the gas over the solution.
$P=K_{H}C$ where
P is the partial pressure of the gas above the solution
$K_H$ is theHenry's Lawconstant for the solution
C is the concentration of the dissolved gas in solution
$C=\frac{P}{K_H}$
C = 2.4 atm/29.76 atm/(mol/L)
C = 0.08 mol/L
since we only have 1 L of water, we have 0.08 mol of $C{O}_2$