Open Question
The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?
9. Solutions
Henry's Law Calculations
Multiple Choice
At 0ºC and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0ºC and 4.00 atm, how many grams of O2 dissolve in 1.0 L of water?
A
0.105 g
B
3.36 g
C
6.72 g
D
4.68 g
Verified step by step guidance1
Identify that this problem involves 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.
Write the formula for Henry's Law: \( S_1/P_1 = S_2/P_2 \), where \( S_1 \) and \( S_2 \) are the solubilities of the gas at pressures \( P_1 \) and \( P_2 \), respectively.
Substitute the known values into the equation: \( 0.84 \, \text{g/L} / 1.00 \, \text{atm} = S_2 / 4.00 \, \text{atm} \).
Solve for \( S_2 \) by multiplying both sides of the equation by 4.00 atm to find the solubility of O2 at the higher pressure.
Interpret the result to determine how many grams of O2 can dissolve in 1.0 L of water at 0ºC and 4.00 atm.
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