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17 October, 08:06

A sample of 4.59 L of CO2 gas has a pressure of 7.56 atm. What volume (in Liters) would the gas occupy if the pressure was reduced to 2.57 atm and the temperature raised from 25.0oC to 39.0oC?

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  1. 17 October, 08:16
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    The answer to your question is V = 14.44 L

    Explanation:

    Data

    Conditions 1 Conditions 2

    V1 = 4.69 L V2 = ?

    P1 = 7.56 atm P2 = 2.57 atm

    T1 = 25°C T2 = 39°C

    Process

    1. - Convert the temperature to °K

    T1 = 25 + 273 = 298°K

    T2 = 39 + 273 = 312 °K

    2. - Find V2 using the combined gas law

    (P1V1) / T1 = (P2V2) / T2

    solve for V2

    V2 = (P1V1T2) / (T1P2)

    substitution

    V2 = (7.56 x 4.69 x 312) / (298 x 2.57)

    Simplify

    V2 = 11062.39 / 765.86

    Result

    V2 = 14.44 L
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