At a fixed temperature, 2 moles of nitrogen gas (N2) are dissolved in water

at a partial pressure of 6 atm. If 4 moles of nitrogen gas (N2) were dissolved

instead, what would the partial pressure be?

A) 3 atm

B) 6 atm

C) 12 atm

D) 24 atm

Click to reveal answer

According to Henry’s law, C = kP where C = concentration of a

dissolved gas, k = Henry’s law constant, and P = partial pressure of the gas. Henry’s

law assumes that temperature remains unchanged, which is the assumption

indicated in this particular scenario.

The initial situation can be described as C = kP or 2 moles N2= k(6 atm). Rearranged,

this means that k = 2 moles N2 / 6 atm. Using this constant value, the partial

pressure of 4 moles of nitrogen can be calculated.

C = (2 moles N2 / 6 atm)(P)

4 moles N2 = (2 moles N2 / 6 atm)(P)

P = 12 atm

B/B Q15 - SA: Digestive system - acid question

If you have any questions or see any issues with this page, please get in touch with matthew.russell@inspiraadvantage.com

Day 110 MCAT Practice Question