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10 April, 04:51

A gas exerts a pressure of 350.0 torr at 20.0 Celsius. What would be the new pressure in atmospheres if the temperature is raised to 40.0 Celsius

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Answers (2)
  1. 10 April, 05:34
    0
    373.88 torr

    Explanation:

    P1 = 350 torr

    T1 = 20°C = (20 + 273.15) K = 293.15K

    P2 = ?

    T2 = 40°C = (40 + 273.15) K = 313.15K

    From pressure law,

    Pressure of a given mass of gas is directly proportional to its temperature.

    P = KT

    K = P / T

    P1 / T1 = P2 / T2

    Solve for P2

    P2 = (P1 * T2) / T1

    P2 = (350 * 313.15) / 293.15

    P2 = 109602.5 / 293.15

    P2 = 373.878 torr

    P2 = 373.88 torr

    The new pressure of the gas would be 373.88 torr.
  2. 10 April, 06:01
    0
    0.49 atm

    Explanation:

    Step 1:

    Data obtained from the question. This includes:

    Initial pressure = 350.0 torr

    Initial temperature (T1) = 20°C

    Final temperature (T2) = 40°C

    Final pressure (P2) = ?

    Step 2:

    Conversion to appropriate unit.

    It is so vital to convert the units of the variable given to the appropriate unit in order to obtain the desired answer in the right unit. This is illustrated below:

    For pressure:

    760 torr = 1 atm

    Therefore, 350 torr = 350/760 = 0.46 atm

    For temperature:

    Temperature (Kelvin) = temperature (celsius) + 273

    T1 = 20°C = 20°C + 273 = 293K

    T2 = 40°C = 40°C + 273 = 313K

    Step 3:

    Determination of the new pressure.

    The new pressure can be obtained by applying the following equation:

    P1/T1 = P2/T2

    P = 0.46 atm

    T1 = 293K

    T2 = 313K

    P2 = ?

    P1/T1 = P2/T2

    0.46 / 293 = P2 / 313

    Cross multiply to express in linear form

    293 x P2 = 0.46 x 313

    Divide both side by 293

    P2 = (0.46 x 313) / 293

    P2 = 0.49 atm

    Therefore, the new pressure is 0.49 atm
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