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2 March, 06:48

A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 313.0 Torr at 45.0 °C. Calculate the value of ΔH°vap for this liquid.

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  1. 2 March, 07:08
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    Given Data:

    P 1=92 torr

    P 2=313

    T 1=296 k

    T 2=318

    Hvap = 47900 Joules

    R=1.99 cal/mole-k

    Using Clausius-Clapeyron equation:

    logP2/P1 = delta H / (2.303*R) * (1/T1-1/T2)

    log 313/92=0.53

    2.303*R = 2.303*1.99

    = 4.5829 cal/mole-k

    1/T1-1/T2=1/296 - 1/318

    = 0.0000233

    delta H = 0.53*4.5829/0.000233

    delta H = 10424.622 cal
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