Question

The Henry’s law constant for \({\bf{CO}}_2\)is \({\bf{3}}{\bf{.4 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}{\bf{ M AT}}{{\bf{M}}^{{\bf{ - 1}}}}\)at 25 °C. What pressure of carbon dioxide is needed to maintain a \({\bf{CO}}_2\)concentration of 0.10 M in a can of lemon-lime soda?

Short answer

The pressure of carbon dioxide needed to maintain the concentration of 0.10M in a can of lemon-lime soda is 2.9atm.

Step-by-step solution

Definition

Henry’s law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid.

Explanation for Ions Interaction

This problem requires the application of Henry’s law.

The governing equation is:

Cg = kPg

C_g= Concentration of a dissolved gas

k = Henry's Law Constant

P_g= Partial pressure of the gas

P_g = C_g/k

P_g = 0.10/o.o34M atm^-1=2.9 atm