Question

At 25 °C and 765 Torr, carbon dioxide has a solubility of 0.0342 M in water. What is its solubility at 25 °C and 1730 Torr?

Answer 1

The solubility of CO2 in water at 25 °C and 1730 Torr is calculated to be 0.0684 M by applying Henry's Law, which infers that solubility is directly proportional to pressure.

Step-by-step explanation:

The question relates to the solubility of CO2 in water under different pressures, commonly understood through Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. Given the initial solubility of CO2 at 765 Torr and 25 °C, we can calculate its solubility at a different pressure, maintaining the same temperature.

According to Henry's Law, if the pressure is doubled (from 765 to 1730 Torr), the solubility will also double. Therefore, at 25 °C and 1730 Torr, the new solubility of carbon dioxide in water would be 0.0342 M × 2 = 0.0684 M.

Answer 2

Answer is: solubility of a carbon dioxide is 0,077 M.
The solubility of a carbon dioxide is directly proportional to the pressure:
p₁ = 765 torr.
p₂ = 1730 torr.
solubility₁ = 0,0342 M.
solubility₂ = ?
p₁/p₂ = solubility₁/solubility₂.
solubility₂ = p₂ · solubility₁ ÷ p₁.
solubility₂ = 1730 torr · 0,0342 M ÷ 765 torr.
solubility₂ = 0,077 M.