A container has a volume of 2.79 L and a pressure of 5.97 atm. If the pressure changes to 1460 mm Hg, what is the container’s new volume?

Boyle's law...... P and V at constant T

P1V1 = P2V2 .............. Boyle's law
V2 = P1V1 / P2 ........... solve for V2
P2 = 5.97 atm x 2.79L / (1460 torr x (1.00 atm / 760 torr))
P2 = 8.67 atm

Here's one of those oddly worded question about "If the pressure changes...." Pressure is a dependent variable. Some independent variable must change in order to change the pressure, something like the volume, temperature or number of moles. Since the moles and temperature are fixed, the volume must be changed in order to change the pressure. The pressure can't change on its own.

Original: P₁ = 5.97 atm = 5.97 × 760 mmHg, V₁ = 2.79 L
New: P₂ = 1460 mmHg, V₂ = ? L

For a fixed amount of gas at constant temperature: P₁V₁ = P₂V₂
Then, V₂ = V₁ × (P₁/P₂)

New volume = (2.79 L) × (5.97 × 760 / 1460) = 8.67 L

The containers volume will be the same if it is a rigid container.! Reducing the pressure will reduce the amount(mols) of gas


The question doesn't say rigid or not so either answer is correct.