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

Answer: (A)

Verified step by step guidance

1. 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.
2. 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.
3. Rearrange the formula to solve for pressure (P): P = C / k.
4. Substitute the given values into the rearranged formula: P = 0.103 M / (1.67 × 10^-4 M • atm^-1).
5. Perform the division to find the pressure in atm, ensuring that units cancel appropriately to leave the result in atm.