Question

A sample of gas has a pressure of 3.6 atmospheres at a temperature of 301 Kelvin. What would be the pressure of the same sample of gas when the temperature is decreased to 285 Kelvin? Show all of the work used to solve this problem.

Answer 1

Given Pressure P1 = 3.6 atm; Pressure P2 = P
Temperature T1 = 301 K; Temperature T2 = 285.K
We have an equation, PV = nRT,
With n and V remains constant pressure is directly proportional to
temperature.
That gives P1 / P2 = T1 / T2 => 3.6 / P = 301 / 285
P = 3.6 x 285 / 301 = 3.4 atm
Pressure P2 = 3.4 atm

Answer 2

Answer is: pressure is 3,40 atm
Gay-Lussac's Law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.
p₁/T₁ = p₂/T₂.
p₁ = 3,6 atm.
T₁ = 301 K.
p₂ = ?.

T₂ = 285 K.

3,6 atm/301 K = p₂/285 K.
3,6 atm · 285 K = 301 K · p₂.

p₂ = 1026 atm · K ÷ 301 K.

p₂ = 3,4 atm