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15 July, 16:17

495 cm3 of oxygen gas and 877 cm3 of nitrogen gas, both at 25.0 C and 114.7 kpa, are injected into an evacuated 536 cm3 flask. Find the total pressure in the flask, assuming the temperature remains constant.

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Answers (2)
  1. 15 July, 16:36
    0
    2.8999 atm

    Explanation:

    Answer:

    Total pressure of the flask is 2.8999 atm.

    Explanation:

    Given dа ta:

    Volume of oxygen (O2) gas = 495 cm3

    = 0.495 L (1 cm³ = 1 mL = 0.001 L)

    Volume of nitrogen (N2) gas = 877 cm3

    = 0.877 L (1 cm³ = 1 mL = 0.001 L)

    volume of falsk = 536 cm3

    = 0.536 L (1 cm³ = 1 mL = 0.001 L)

    Temperature = 25 °C

    T = (25°C + 273.15) K

    = 298.15 K

    Pressure = 114.7 kPa

    = 114.700 Pa

    Pressure (torr) = 114,700 / 101325

    = 1.132 atm

    Formula:

    PV=nRT (ideal gas equation)

    P = pressure

    V = volume

    R (gas constnt) = 0.0821 L. atm/K. mol

    T = temperature

    n = number of moles for both gases

    Solution:

    Firstly we will find the number of moles for oxygen and nitrogen gas.

    For Oxygen:

    n = PV / RT

    n = 1.132 atm * 0.495 L / 0.0821 L. atm/K. mol * 298.15 K

    = 0.560 / 24.47

    = 0.0229 moles

    For Nitrogen:

    n = PV / RT

    n = 1.132 atm * 0.877 / 0.0821 L. atm/K. mol * 298.15 K

    n = 0.992 / 24.47

    = 0.0406

    Total moles = moles for oxygen gas + moles for nitrogen gas

    = 0.0229 moles + 0.0406 moles

    n = 0.0635 moles

    Now put the values in formula

    PV=nRT

    P = nRT / V

    P = 0.0635 * 0.0821 L. atm/K. mol * 298.15 K / 0.536 L

    P = 1.554 / 0.536

    P = 2.8999 atm

    Total pressure in the flask is 2.8999 atm, while assuming the temperature constant.
  2. 15 July, 17:36
    0
    Total pressure of the flask is 2.8999 atm.

    Explanation:

    Given dа ta:

    Volume of oxygen (O2) gas = 495 cm3

    = 0.495 L (1 cm³ = 1 mL = 0.001 L)

    Volume of nitrogen (N2) gas = 877 cm3

    = 0.877 L (1 cm³ = 1 mL = 0.001 L)

    volume of falsk = 536 cm3

    = 0.536 L (1 cm³ = 1 mL = 0.001 L)

    Temperature = 25 °C

    T = (25°C + 273.15) K

    = 298.15 K

    Pressure = 114.7 kPa

    = 114.700 Pa

    Pressure (torr) = 114,700 / 101325

    = 1.132 atm

    Formula:

    PV=nRT (ideal gas equation)

    P = pressure

    V = volume

    R (gas constnt) = 0.0821 L. atm/K. mol

    T = temperature

    n = number of moles for both gases

    Solution:

    Firstly we will find the number of moles for oxygen and nitrogen gas.

    For Oxygen:

    n = PV / RT

    n = 1.132 atm * 0.495 L / 0.0821 L. atm/K. mol * 298.15 K

    = 0.560 / 24.47

    = 0.0229 moles

    For Nitrogen:

    n = PV / RT

    n = 1.132 atm * 0.877 / 0.0821 L. atm/K. mol * 298.15 K

    n = 0.992 / 24.47

    = 0.0406

    Total moles = moles for oxygen gas + moles for nitrogen gas

    = 0.0229 moles + 0.0406 moles

    n = 0.0635 moles

    Now put the values in formula

    PV=nRT

    P = nRT / V

    P = 0.0635 * 0.0821 L. atm/K. mol * 298.15 K / 0.536 L

    P = 1.554 / 0.536

    P = 2.8999 atm

    Total pressure in the flask is 2.8999 atm, while assuming the temperature constant.
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