There is 50.0 mL of a gas at a temperature of 5°C. Its pressure is 760 mm Hg. What temperature is needed

to change the volume to 55mL and the pressure to 780 mm Hg?

41°C

Explanation:

Ideal gas law:

PV = nRT

where P is absolute pressure,

V is volume,

n is number of moles,

R is universal gas constant,

and T is absolute temperature.

n is held constant, so:

P₁V₁ / T₁ = P₂V₂ / T₂

Given:

P₁ = 760 mmHg

V₁ = 50.0 mL

T₁ = 5°C = 278 K

P₂ = 780 mmHg

V₂ = 55 mL

Find: T₂

(760 mmHg) (50.0 mL) / (278 K) = (780 mmHg) (55 mL) / T

T = 314 K

T = 41°C