If a 1.00 L sample of hydrogen gas has a pressure of 790 torr at a temperature of 1.0 °C, what would be its new volume if the temperature increased to 310 °C and the pressure increased to 5837 torr?

V₂ = 0.28 L

Explanation:

Given data:

Initial volume = 1.00 L

Initial pressure = 790 torr (790/760 = 1 atm)

Initial temperature = 1.0 °C (1.0 +273 = 274 K)

Final temperature = 310°C (310+273 = 583 K)

Final volume =?

Final pressure = 5837 torr (5837/760 = 7.7 atm)

Solution:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 1 atm × 1.0 L × 583 k / 274 k × 7.7 atm

V₂ = 583  / 2109.8

V₂ = 0.28 L

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