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20 February, 03:58

The pressure of a 70.0L sample of gas is 600 mm Hg at 20.0C. If the temperature drops to 15.0C and the volume expands to 90.0L, what will the pressure of the gas be?

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  1. 20 February, 04:13
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    458.7 mmHg

    Explanation:

    Step 1:

    Data obtained from the question. This includes:

    Initial volume (V1) = 70L

    Initial pressure (P1) = 600 mmHg

    Initial temperature (T1) = 20°C

    Final temperature (T2) = 15°C

    Final volume (V2) = 90L

    Final pressure (P2) = ... ?

    Step 2:

    Conversion of celsius temperature to Kelvin temperature.

    This is illustrated below:

    T (K) = T (°C) + 273

    Initial temperature (T1) = 20°C

    Initial temperature (T1) = 20°C + 273 = 293K

    Final temperature (T2) = 15°C

    Final temperature (T2) = 15°C + 273 = 288K

    Step 3:

    Determination of the new pressure of the gas.

    The new pressure of the gas can be obtained by using the general gas equation as shown below:

    P1V1/T1 = P2V2/T2

    600 x 70/293 = P2 x 90/288

    Cross multiply to express in linear form

    P2 x 90 x 293 = 600 x 70 x 288

    Divide both side by 90 x 293

    P2 = (600 x 70 x 288) / (90 x 293)

    P2 = 458.7 mmHg

    Therefore, the new pressure of the gas is 458.7 mmHg
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