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9 August, 18:39

There is 50.0 mL of a gas at a temperature of 5°C. Its pressure is 760 mm Hg. What temperature is needed

to change the volume to 55mL and the pressure to 780 mm Hg?

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Answers (1)
  1. 9 August, 22:00
    0
    41°C

    Explanation:

    Ideal gas law:

    PV = nRT

    where P is absolute pressure,

    V is volume,

    n is number of moles,

    R is universal gas constant,

    and T is absolute temperature.

    n is held constant, so:

    P₁V₁ / T₁ = P₂V₂ / T₂

    Given:

    P₁ = 760 mmHg

    V₁ = 50.0 mL

    T₁ = 5°C = 278 K

    P₂ = 780 mmHg

    V₂ = 55 mL

    Find: T₂

    (760 mmHg) (50.0 mL) / (278 K) = (780 mmHg) (55 mL) / T

    T = 314 K

    T = 41°C
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