Chapter 21, Problem 7STP

Interpretation Introduction

Interpretation:

The amount of dissolved ${\text{CO}}_{\text{2}}$ should be calculated when the pressure is increased to 1.35 atm and temperature remains same.

1. 2.23 g/L
2. 1.27 g/L
3. 0.785 g/L
4. 0.431 g/L

Concept introduction:

According to Henry’s Law, the solubility of a gas is directly related with the pressure of a gas implies with increase in pressure, the solubility of a gas also increases.

Answer to Problem 7STP

The amount of dissolved ${\text{CO}}_{\text{2}}$ is 2.23 g/Lwhen the pressure is increased to 1.35 atm and temperature remains same. Thus, option (A) is correct.

Explanation of Solution

Given information:

Initial pressure = 1.00 atm

Temperature = $\text{20}°\text{C}$

Mass of ${\text{CO}}_{\text{2}}$ = 1.72 g

Volume of water = 1 L

Final Pressure = 1.35 atm

It is given that at 1.00 atm, 1.72 g of carbon dioxide is dissolved in one liter of water. As the pressure increases to 1.35 atm, the amount of carbon dioxide also increases.

Now,

(A)Since, the solubility of a gas increases with increase in pressure. Also, concentration of dissolved carbon dioxide must be greater than the initial concentration as the pressure increases.

2.23 g/L>1.72 g/L, thus, amount of dissolved carbon dioxide is 2.23 g/L.

Hence, option (A) is correct.

Other given options are not possible as values are less than the original or initial concentration.