Multiple Choice
The Henry's law constant at 25 °C for CO₂ in water is 0.035 M/atm. What is the solubility of CO₂, in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 2.3 atm?
14. Solutions
Henry's Law Calculations
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Henry's Law Constant for nitrogen in water is 1.67 × 10-4 M • atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?
A
617 atm
B
1.72 × 10–5 atm
C
1.62 × 10–3 atm
D
778 atm
Verified step by step guidance1
Identify the given values: Henry's Law Constant (k) is 1.67 × 10-4 M • atm-1 and the concentration of nitrogen (C) is 0.103 M.
Recall Henry's Law, which states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is C = kP, where C is the concentration, k is the Henry's Law constant, and P is the pressure.
Rearrange the formula to solve for pressure (P): P = C / k.
Substitute the given values into the rearranged formula: P = 0.103 M / (1.67 × 10-4 M • atm-1).
Perform the division to find the pressure in atm, ensuring that units cancel appropriately to leave the result in atm.
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