Henry's Law Overview/Introduction
In this assignment, you will determine the solubility of various gases using Henry's Law. This will help you understand how temperature, pressure, and the solubility coefficient contribute to the dissolving of a gas.
Directions:
Complete the problems for each section. If you used steps to complete the calculations or determine the answer, please include them with your answer. All answers and work shown should be neat, clear, and legible.
- How many grams of oxygen can be dissolved in 1 L of water at 20 °C if the oxygen pressure is 2.00 atm (kO2 = 1.38 x 10^-3 M/atm)?
- If 0.55 g of a gas dissolves in 1.0 L of water at 2 atm of pressure, how much will dissolve at 4.5 atm of pressure?
- An unopened soda has an aqueous concentration of CO2 at 25 °C equal to 0.05 g/L. What is the partial pressure of CO2 in the can if kCO2 = 0.034 M/atm?
- Carbon monoxide gas is dissolved in water at 25 °C and 0.03 atm. If the constant for this system is 5.80 x 10^-4 M/atm, what is the solubility of CO?
- If 0.68 g of a gas at 5.00 atm dissolves in 1.0 L of water at 25 °C, how much will dissolve in 1.0 L of water at 8.00 atm if the temperature remains constant?