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 85 ∘ c? express your answer with the appropriate units.

Question

Aylin Moran

Physics

21 October, 19:46

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 85 ∘ c? express your answer with the appropriate units.

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Answers (1)

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Monserrat Johnson · Answer 1

Gay-Lussac's law described the relation between the pressure and the temperature of a gas at a certain volume.

His law states that: "At constant volume, the pressure of the gas is directly proportional to the temperature."

P/T = constant

This can be written as:

P1 / T1 = P2 / T2 where:

P1 is the initial pressure = 2.1 atm

T1 is the initial temperature = 21 + 273 = 294 degrees kelvin

P2 is the final pressure that we need to calculate

T2 is the final temperature = 85 + 273 = 358 degrees kelvin

Substitute with the givens in the above relation to get the value of P2 as follows:

(2.1) / (294) = P2 / (358)

P2 = 358 * (2.1/294)

P2 = 2.557 atm

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 85 ∘ c? express your answer with the appropriate units.

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 85 ∘ c? express your answer with the appropriate units.