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College chemistry

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How much heat (in kJ) is evolved in converting 1.00 mol of steam at 130.0 C to ice at -50.0 C? The heat capacity of steam is 2.01 J/g*C and of ice is 2.09 J/g*C.

  • College chemistry -

    You must go through all of the steps from steam at 130 to ice at -50.
    q to move steam at 130 to steam at 100.
    q1 = mass x specific heat x delta T.

    q to convert steam at 100 to liquid water at 100.
    q2 = mass x heat of vaporization.

    q to move water at 100 to water at zero.
    q3 = mass x specific heat x delta T.

    q to convert water at zero to ice at zero.
    q4 = mass x heat of fusion.

    q to move ice at zero to ice at -50.
    q5 = mass x specific heat x delta T.

    Then total q =
    q1+q2+q3+q4+q5.
    I notice your specific heats are listed in joules so your answer will come out in Joules and you must convert to kJ since the problem asks for kJ.

  • College chemistry -

    55.078

  • College chemistry -

    57 kj

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