Hydrogen gas at a temperature of 22.0 degrees C that is confined in a 5.00 L cylinder exerts a pressure of 4.20 atm. If the gas is released into a 10.0 L reaction vessel at a temperature of 33.6 degrees C, what will be the pressure inside the reaction vessel?

P₂ = 2.18 atm

Explanation:

Given data:

Initial temperature of gas = 22°C

Initial volume of gas = 5.00 L

Initial pressure = 4.20 atm

Final volume = 10 L

Final temperature = 33.6°C

Final pressure = ?

Solution:

First of all we will convert the temperature into kelvin.

Initial temperature of gas = 22°C (22+273.15 = 295.15 K)

Final temperature = 33.6°C (33.6+273.15 = 306.75 k)

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

P₂ = P₁V₁ T₂/ T₁ V₂  

P₂ = 4.2  atm × 5 L × 306.75 K / 295.15 K × 10 L  

P₂ = 6441.75 atm .L. K / 2951.5 K.L

P₂ = 2.18 atm

the maximum mass of nh3 is nh3 in grams