A system absorbs 194 kj of heat and the surroundings do 120 kj of work on the system. internal eneergy change

Question

A system absorbs 194 kj of heat and the surroundings do 120 kj of work on the system. internal eneergy change

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2022-04-20T10:42:36+00:00 1 Answer 0

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  1. Kaylee
    0
    2022-04-20T10:43:46+00:00

    We can solve the problem by using the first law of thermodynamics, which states that:
    [tex]Delta U = Q-W[/tex]
    where
    [tex]Delta U[/tex] is the change in internal energy of the system
    Q is the heat absorbed by the system
    W is the work done by the system

    In our problem, the heat absorbed by the system is Q=+194 kJ, while the work done is W=-120 kJ, where the negative sign means the work is done by the surroundings on the system. Therefore, the variation of internal energy is
    [tex]Delta U= Q-W=+194 kJ – (-120 kJ)=+314 kJ[/tex]

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