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25 August, 01:54

A sample of gas occupies 40.0 mL at - 123°C. What volume does the sample occupy at 27°C if the pressure is held constant? V1T2 = V2T1 Don't forget to convert temperature to kelvin! Group of answer choices 8.80 mL 20.0 mL 80. ML 182 mL

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  1. 25 August, 02:24
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    80mL

    Explanation:

    Step 1:

    Data obtained from the question.

    Initial Volume (V1) = 40mL

    Initial temperature (T1) = - 123°C

    Final temperature (T2) = 27°C

    Final volume (V2) = ... ?

    Step 2:

    Conversion of celsius temperature to Kelvin temperature.

    T (K) = T (°C) + 273

    Initial temperature (T1) = - 123°C =

    -123°C + 273 = 150K

    Final temperature (T2) = 27°C = 27°C + 273 = 300K

    Step 3:

    Determination of the final volume.

    This can be obtained as follow:

    V1/T1 = V2/T2

    Initial Volume (V1) = 40mL

    Initial temperature (T1) = 150K

    Final temperature (T2) = 300

    Final volume (V2) = ... ?

    V1/T1 = V2 / T2

    40/150 = V2 / 300

    Cross multiply

    150 x V2 = 40 x 300

    Divide both side by 150

    V2 = (40 x 300) / 150

    V2 = 80mL

    Therefore, the new volume of the gas is 80mL
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