Question

Part A

The pressure inside a hydrogen-filled container was 2.10 atm at 21 ?C. What would the pressure be if the container was heated to 93?C ?

Part A The pressure inside a hydrogen-filled container was 2.10 atm at 21 ?C. What would the pressure be if the container was heated to 93?C ? Express your answer numerically in atmospheres. Part B At standard temperature and pressure (0 ?C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 65?C ?

Answer 1

Part-A :

Ideal gas equation is PV = nRT

Where P-Pressure , V -Volume ; n- number of moles ; T- temperature in kelvin ; R- gas constant

For two cases where the amount of gas will not change,

        Since volume of the container remains constant

Where

P₁ = initial pressure = 2.10 atm

T₁ = initial temperature =21 ⁰C = 21 + 273 = 294 K         

P₂ = final pressure = ?

T₂ = final temperature = 93 ⁰C = 93 + 273 = 366 K

Plug the values we get

Part-B :

Ideal gas equation is PV = nRT

Where P-Pressure , V -Volume ; n- number of moles ; T- temperature in kelvin ; R- gas constant

For two cases where the amount of gas will not change,

                 Since pressure remains constant

Where

T₁ = initial temperature =0 ⁰C = 0 + 273 = 273 K         

T₂ = final temperature = 65 ⁰C = 65 + 273 = 338 K

V₁ = initial volume = 22.4L

V₂ = final volume = ?

Plug the values we get