A 3.0 l sample of helium gas is stored in a rigid, sealed container at 25 °c and 1.0 atm pressure. the temperature is increased to 125 °c. what is the new pressure of the gas?

Question

Haylie Riley

Chemistry

27 January, 09:30

A 3.0 l sample of helium gas is stored in a rigid, sealed container at 25 °c and 1.0 atm pressure. the temperature is increased to 125 °c. what is the new pressure of the gas?

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Gideon Maxwell · Answer 1

Assume ideal gas for simplicity so we could use the ideal gas equation. The hint words in here are the 'rigid, sealed container'. It means the volume is constant. So, we will use Gay-Lussac's Law.

T₁/P₁ = T₂/P₂

We have to solve for P₂. The solution is as follows:

(25 + 273 K) / 1 atm = (125 + 273 K) / P₂

Solving for P₂,

P₂ = 1.34 atm