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Natural gas is almost entirely methane, CH4. What volume of natural gas at 20 C and 1.00 atm pressure is required to heat one quart of water from 20 C to 100 C? The density of methane at 20 C is 0.665 g/mL. The reaction for the combustion of methane is
CH4 (g) + 2 O2 (g) --> CO2 + 2 H2O (g)

  • Chemistry - ,

    You have everything here except the heat of combustion of CH4.

  • Chemistry - ,

    I have no idea how to solve for the volume of methane. Any help?

  • Chemistry - ,

    Yes BUT you need the heat of combustion of CH4 to know howmuch heat it produces.

    How much heat do you need? (1 qt H2O = 0.946 L and if the density of H2O is 1.00 g/mL that is 946 g)That's
    q = 946 g H2O x specific heat H2O x (Tfinal-Tinitial). Let's suppose this is y joules.

    g CH4 needed to produce y joules is
    16 g CH4 x (y joules/heat combustion) = g CH4

    Convert g CH4 to cc methane using the density. That is the volume.
    You don't have heat combustion CH4, density of H2O (which I assumed as 1.00 g/mL), or specific heat H2O (which is 4.184 J/g or 1 cal/g)

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