Question

A fixed quantity of gas at 21 ∘C exhibits a pressure of 750 torrand occupies a volume of 5.42 L .

A) Calculate the volume the gas will occupy if the pressure is increased to 1.89 atm while the temperature is held constant.

B) Calculate the volume the gas will occupy if the temperature is increased to 175 ∘C while the pressure is held constant.

Answer 1

Given

A gas at 21∘C exhibits a pressure of 750 torr and occupies a volume of 5.42 L

A)

pressure is increased to 1.89 atm, temperature is held constant

1 atm = 760 torr

1.89 atm = 1.89 atm*760 torr/1 atm

= 1436.4 torr

Applying boyles law(as temperature is held constant)

P1V1 = P2V2

750 torr *5.42 L = 1436.4 torr*V2

==>V2 = 2.83 L

volume of the gas = 2.83 L

B)

temperature is increased to 175 ∘C, pressure is held constant.

21∘C = (21+273)K = 294K

175∘C = (175+273)K = 448K

Applying Charles law(as pressure is held constant)

V1/T1 = V2/T2

5.42 L/(294K) = V2/448K

V2 = 8.26 L

volume of the gas = 8.26 L