A mixture of methane and water vapor pressure is passed over a nickel catalyst a

Question

A mixture of methane and water vapor pressure is passed over a nickel catalyst at 1000K. The emerging gas is collected in a 5.00L flask and is found to contain 8.62g of carbon monoxide, 2.60g of hydrogen gas, 43.0g of methane, and 48.4g of water vapor. Assuming that equilibrium has been reached, calculate Kc and Kp for the reaction.

Explanation / Answer

Get balanced reaction: CH4(g) + H2O(g) -> CO(g) + 3H2(g) Find the MOLAR (moles/Liter) concentrations of respective substances: [CO]: 8.62/(28.01)=.301 mol/5L [H2]: 2.60/(2.02)=1.287 mol/5L [CH4]: 43.0/16.04=2.681/5L [H2O]: 48.4/18.02=2.686/5L Kc= [H2]^3 X [CO] / ( [CH4] X [H2O]) = 3.5642 X 10^(-6) Kp=Kc(RT)^(?n), ?n is the change in moles of gas (3 H2 + 1CO) - (1 CH4 + 1 H2O) =3.5642 X 10^(-6) (.0821 X 1000) ^ (4-2) =3.5642 X 10^(-6) (.0821 X 1000)^(2) =.0240

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