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30 March, 08:56

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?

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  1. 30 March, 10:42
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    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
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