How many liters if hydrogen (at 744 torr & 24°C) react with 23.0 g of propylene?

Update:

I still cannot figure this out

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  • 6 months ago
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    Propene + hydrogen ➜ propane

    C₃H₆ + H₂ ➜ C₃H₈

    23 g of H₂ / 2g/mol = 11.5 mol

    mole ratio says 1:1, so 11.5 mol of C₃H₆

    now many liters of hydrogen (at 744 torr & 24°C)

    V = nRT/P = (11.5)(62.36)(273.16+24) / (744) = _____ L

    (you have a calculator)

    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

  • Anonymous
    6 months ago

    1 mole of propylene will react with 1 mole of H2.

    Moles of propylene =? (About 1/2)

     

    Use the ideal gas equation to find the volume of hydrogen, V = nRT/P.  About 10.

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