659 mmHg and 283 K

Question

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 ∘C. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, if the amount of gas does not change?

Answer 1

Given:

V1 (initial volume) = 735 ml

P1 (initial pressure) = 1.20 atm

T1 (initial temperature) = 112ºC + 273 = 385K

P2 (final pressure) = 659 mm Hg x 1 atm/760 mm Hg = 0.867 atm (change to atm to be consistent w/ P1)

T2 (final temperature) = 283K

Asked to find:

V2 (final volume)

This involves the use of the combined gas law: P1V1/T1 = P2V2/T2

Rearrange and solve for V2: V2 = P1V1T2 / P2T1

Plug in the above values and solve. Answer will be in milliliters because V1 is in milliliters