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23 February, 13:10

A sample of nitrogen gas in a 1.59-L container exerts a pressure of 1.47 atm at 26 ∘C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 371 ∘C?

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  1. 23 February, 14:05
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    New pressure is 3.16 atm

    Explanation:

    Let's apply the Gay Lussac law for this which states the pressure of a fixed volume of a gas is directly proportional to its temperature.

    As the T° raises, the pressure raises too.

    Is the T° decreases, the pressure will decrease too.

    P₁ / T₁ = P₂ / T₂

    First of all, let's convert the T° to aboslute values:

    26°C + 273 = 299 K

    371°C + 273 = 644 K

    1.47 atm / 299 K = P₂ / 644 K

    (1.47 atm / 299 K). 644 K = P₂

    P₂ = 3.16 atm
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