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23 March, 13:40

What is the pressure of 62.76 g of carbon dioxide (CO2) gas if it occupies a volume of

35,000 mL at standard temperature?

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Answers (2)
  1. 23 March, 14:59
    0
    The pressure of the carbon dioxide (CO2) gas is 0.913 atm

    Explanation:

    Step 1: Data given

    Mass of carbon dioxide (CO2) = 62.76 grams

    Molar mass of carbon dioxide (CO2) = 44.01 g/mol

    Volume = 35000 mL = 35 L

    Standard temperature = 273 K

    Step 2: Calculate moles CO2

    Moles CO2 = mass CO2 / molar mass

    Moles CO2 = 62.76 grams / 44.01 g/mol

    Moles CO2 = 1.426 moles

    Step 3: Calculate the pressure

    p*V = n*R*T

    ⇒with p = the pressure of the gas

    ⇒with V = the volume of the gas = 35 L

    ⇒with n = the moles of the gas = 1.426 moles

    ⇒with R = the gas constant = 0.08206 L*atm/mol * K

    ⇒with T = the temperature = 273 K

    p = (n*R*T) / V

    p = (1.426 * 0.08206 * 273) / 35

    p = 0.913 atm

    The pressure of the carbon dioxide (CO2) gas is 0.913 atm
  2. 23 March, 15:36
    0
    P = 995.6 atm

    Explanation:

    assuming ideal gas:

    PV = RTn

    ∴ Tst = 25°C ≅ 298 K

    ∴ V = 35.00 mL = 0.035 L

    ∴ molar mass CO2 = 44.01 g/mol

    ∴ mass CO2 (g) = 62.76 g

    ⇒ mol CO2 (g) = (62.76 g) * (mol/44.01 g) = 1.426 mol

    ∴ R = 0.082 atm. L/K. mol

    ⇒ P = RTn/V

    ⇒ P = ((0.082 atm. L/K. mol) * (298 K) * (1.426 mol)) / (0.035 L)

    ⇒ P = 995.6 atm
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