A volume of 2.15 mL of Oxygen was collected in the lab at a temperature of 17 °C and 740.2 mmHg. After a day, the volume of the gas has become 2.21 mL and the barometer reading (for air pressure) had not changed. What is the new temperature in the lab (in °C)?

The new temperature (T₂) in the lab = 25.09 °C

Given

V₁=2.15 ml

T₁ = 17 + 273 = 290 K

P = 740.2 mmHg

V₂ = 2.21 ml

Required

The new temperature (T₂)

Solution

Charles's Law

When the gas pressure is kept constant, the gas volume is proportional to the temperature

Input the value :

T₂=(T₁.V₂)/V₁

T₂=(290 K x 2.21 ml)/2.15 ml

T₂=298.09 K = 25.09 °C

c, liquids evaporate, creating a gas