A container of oxygen gas is at STP. If this sample is put into an oven at 280 C, what would its pressure be, in atmospheres?

Question

A container of oxygen gas is at STP. If this sample is put into an oven at 280 C, what would its pressure be, in atmospheres?

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Thông Đạt 5 years 2021-07-30T21:02:34+00:00 2 Answers 33 views 0

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  1. Helga
    0
    2021-07-30T21:03:44+00:00
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    Answer:

    \boxed {\boxed {\sf P_2=2.03 \ atm}}

    Explanation:

    We are concerned with the variables of temperature and pressure, so we use Gay-Lussac’s Law, which states the temperature of a gas is directly proportional to the pressure. The formula is:

    \frac{P_1}{T_1}=\frac{P_2}{T_2}

    We know that the container of gas begins at standard temperature and pressure (STP). This is 1 atmosphere of pressure and 273 Kelvin.

    \frac { 1 \ atm}{ 273 \ K} = \frac{P_2}{T_2}

    We know the gas is put into an oven at 280 degrees Celsius. We can convert this to Kelvin.

    • K= °C + 273.15
    • K= 280 +273.15
    • K= 553.15

    \frac { 1 \ atm}{ 273 \ K} = \frac{P_2}{553.15 \ K}

    We are solving for the new pressure, so we must isolate the variable P₂. It is being divided by 553.15 Kelvin. The inverse of division is multiplication, so we multiply both sides by 553.15 K

    553.15 \ K *\frac { 1 \ atm}{ 273 \ K} = \frac{P_2}{553.15 \ K} * 553.15 \ K

    553.15 \ K *\frac { 1 \ atm}{ 273 \ K}= P_2

    The units of Kelvin cancel.

    553.15 *\frac { 1 \ atm}{ 273 }= P_2

    2.02619047619 \ atm = P_2

    Rounded to the nearest hundredth:

    2.03 \ atm \approx P_2

    The new pressure is approximately 2.03 atmospheres.

  2. ngochoa
    0
    2021-07-30T21:04:24+00:00
    Reply



    Explanation:


    Step 1:


    Data obtained from the question. This include the following:


    Initial pressure (P1) = 1atm


    Initial temperature (T1) = 0°C = 0°C + 273 = 273K


    Final temperature (T2) = 280°C = 280°C + 273 = 553K


    Final pressure (P2) =…?


    Step 2:


    Determination of the new pressure of the gas.


    Since the volume of the gas is constant, the following equation:


    P1/T1 = P2/T2


    will be used to obtain the pressure. This is illustrated below:


    P1/T1 = P2/T2


    1/273 = P2 / 553


    Cross multiply


    273x P2 = 553


    Divide both side by 273


    P2 = 553/273


    P2 = 2.03atm


    Therefore, the new pressure of the gas will be 2.03atm

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