CHemistry

posted by .

CH4(g) + CO2(g) <--> 2CO(g) + 2H2(g)
Kp = 4.5 x 10^2 at 825 K

An 85.0 L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K.

Assuming ideal gas behavior, calculate the mass of H2 present in the reaction mixture at equilibrium.

  • CHemistry -

    What is the percent yield of the reaction under these conditions?

  • CHemistry -

    Convert 22.3 kg CH4 to moles.
    Convert 55.4 kg CO2 to moles.
    Using PV = nRT convert moles of both CH4 and CO2 to pressure in the 85 L container. Then set up an ICE chart, substitute into the Kp expression, and solve.
    After you know x (if that's what you call the unknown), that will be partial presure CO and H2. Use PV = nRT to calculate n and go from there.
    percent yield = (mass H2/theoretical yield)*100

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Which pair of molecules has the strongest dipole-dipole interactions?
  2. chemistry

    CH4 + 2O2 = CO2 + 2H2O Starting with 13.6 g of CH4, calculate the mass in grams of CO2 produced if there is enough O2 gas to react with all of the CH4
  3. Chemistry

    which conversion factor do you use to first calculate the number of grams of CO2 produced by tge reaction of 50.6 CH with O2?
  4. Chemistry

    I am having such a hard time approaching this problem. It would be great if you can help me. 1.0 mole of CH4 react with 1.0 mole of O2 in a sealed container. (a) When the reaction is complete, what is the container?
  5. Chemistry

    I am having such a hard time approaching this problem. It would be great if you can help me. 1.0 mole of CH4 react with 1.0 mole of O2 in a sealed container. (a) When the reaction is complete, what is the container?
  6. chemistry

    Nitric oxide (NO) can be removed from gas-fired power-plant emissions by reaction with methane as follows: CH4(g) + 4NO(g) --> 2N2(g) + CO2(g) + 2H2O(g) Complete the equation relating the rates for each of the following: a) the …
  7. chemistry

    When 85.0 g of CH4 are mixed with 160. g of O2 the limiting reactant is __________. CH4 + 2O2 ¨ CO2 + 2H2O A) CH4 B) O2 C) CO2 D) H2O
  8. green valley college

    the principal constituents of natural gas is methane which burns in air according to the reaction CH4+O2=CO2+H2O How many grams of CO2 is produced when you have 50g of both CH4 and O2 what is the limiting reactant?
  9. help

    Methane, CH4, burns in oxygen gas to form water and carbon dioxide. What is the correct balanced chemical equation for this reaction?
  10. chemistry

    The combustion of 1.210 g of a mixture of CH4 and C2H6 gives 3.372 g of CO2 I have to determine the composition of the mixture (mastic %) and molar fraction of CH4 in the mixture CH4 + C2H6: CO2 + 2H2O C2H6 + O2: CO2 + H2O CH4 + C2H6 …

More Similar Questions