ne mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 liters against a constant external pressure of 1.00 atm.

Question

ne mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem.

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Yến Oanh 1 week 2021-07-22T06:03:55+00:00 1 Answers 0 views 0

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    2021-07-22T06:05:36+00:00

    Answer:

    Complete question

    One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T= 300 K:

    1 L•atm = 101.3 J)

    Explanation:

    Given that,

    Number of mole

    n = 1 mole

    Initial volume

    Vi = 1 litre

    Final Volume

    Vf = 8.41 litre

    Constant Pressure

    P = 1 atm

    Work done in Joule?

    Work done under constant pressure is given as

    W = P∆V

    W = P(Vf—Vi)

    W = 1 atm × (8.41—1) litre

    W = 1 atm × 7.41 litre

    W = 7.41 Litre•atm

    Given that,

    1 Litre•atm = 101.3J

    Then,

    W = 7.41 Litre•atm × 101.3J/Litre•atm

    W = 750.633 J

    W ≈ 751J

    Then the work done on the surrounding is approximately

    751 joules

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