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 dа ta:

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