Question

Determine the solubility of CO₂ in soda water at 25°C if the pressure of CO₂ is 5.2 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 x 10⁻² M/atm.

a) 0.15 M
b) 0.57 M
c) 0.65 M
d) 0.18 M
e) 0.29 M

Answer 1

The solubility of CO₂ in soda water at 25°C under a pressure of 5.2 atm is calculated using Henry's Law. With the given Henry's Law constant of 3.4 x 10⁻² M/atm, the solubility is 0.1768 M, which rounds to 0.18 M, the correct answer.

Step-by-step explanation:

To determine the solubility of CO₂ in soda water at 25°C when pressure of CO₂ is 5.2 atm and given the Henry's law constant for carbon dioxide in water at this temperature is 3.4 x 10⁻² M/atm, we use Henry's Law. According to Henry's Law, the solubility of a gas in a liquid at a particular temperature is directly proportional to the partial pressure of the gas above the liquid. So, we can calculate the solubility (S) using the following equation:

S = kH × P

Where:

• S is the solubility of the gas (M)
• kH is the Henry's Law constant (M/atm)
• P is the partial pressure of the gas (atm)

Substituting the given values:

S = (3.4 x 10⁻² M/atm) × (5.2 atm)

S = 0.1768 M

Therefore, the closest option to the calculated solubility is 0.18 M, which makes option d) 0.18 M the correct answer.