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18 April, 22:39

A gas is contained in a cylinder with a volume of 2.9 L at a temperature of 32.7oC and a pressure of 645.3 torr. The gas is then compressed to a volume of 0.23 L, and the temperature is raised to 894.7oC. what is the new pressure of gas (in atm)

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  1. 19 April, 00:12
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    Answer: 41 atm

    Explanation:

    Given that:

    Original Volume of gas V1 = 2.9L

    Temperature T1 = 32.7°C

    Convert Celsius to Kelvin

    (32.7°C + 273 = 305.7K)

    Pressure P1 = 645.3 torr

    New Volume V2 = 0.23 L

    New temperature T2 = 894.7°C

    Convert Celsius to Kelvin

    (894.7°C + 273 = 1167.7K)

    New pressure = ?

    Then, apply the combined gas equation

    (P1V1) / T1 = (P2V2) / T2

    (645.3 torr x 2.9L) / 305.7K = (P2 x 0.23L) / 1167.7K

    1871.37 / 305.7 = 0.23P2 / 1167.7

    To get P2, Cross multiply

    1871.37 x 1167.7 = 305.7 x 0.23P2

    2185198.749 = 70.311P2

    Divide both sides by 70.311

    2185198.749/70.311 = 70.311P2/70.311

    31079.045 torr = P2

    Now, convert pressure in torr to atmosphere

    Since 760 torr = 1 atm

    31079.045 torr = Z

    cross multiply

    760 torr x Z = 31079.045 torr x 1 atm

    Z = 31079.045 torr / 760 torr

    Z = 40.89 atm (Round to the nearest whole number as 41 atm)

    Thus, new pressure of gas is 41 atm
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