An ideal gas at 10.3 °C and a pressure of 2.48 x 10^5 Pa occupies a volume of 3.12 m3. ?

(a) How many moles of gas are present? (b) If the volume is raised to 5.45 m3 and the temperature raised to 25.6 °C, what will be the pressure of the gas?

1 Answer

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  • 1 month ago

    2.48e5 Pa = 248 kPa

    3.12 m³ = 3120 L

    10.3°C = 283.46 K

    n = PV/RT = (248)(3120) / (8.314)(283.46) = 328 mol

    P₂ = P₁V₁T₂/V₂T₁ = (248)(3.12)(25.6+273.16) / (5.45)(8.314) = _____ kPa

      (you have a calculator)

    Combined Gas law

    P₁V₁/T₁ = P₂V₂/T₂

    Ideal gas law

    PV = nRT

    n = number of moles

    R = gas constant = 0.08206 (atm∙L)/(mol∙K)

                       8.314 L∙kPa/mol∙K

                       0.08314 L∙bar/mol∙K

                       62.36 L∙torr/mol∙K

                       62.36 L∙mmHg/mol∙K

    T = temperature in kelvins

    P = absolute pressure in atm, kPa, bar, torr

    V = volume in liters

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