Problem 2

Steam reforming of methane is used extensively in the petroleum industry to generate hydrogen gas.  If the reaction is assumed to be in equilibrium

H2O (g) + CH4 (g) 3H2 (g) + CO (g)

then what is K at 1000 șC if equal concentrations of water and methane of 0.5 mol/L are fed into a reactor, and in the product stream the concentration of CO (g) is 0.221 mol/L?

1. To solve this problem you should use an IRE table something like the following.   a) Complete the reaction row with appropriate values, then press the [Check R] button.  b) Complete the equilibrium row with the appropriate values, then press the [Check E] button.

H2O (g) + CH4 (g)

3H2 (g) + CO (g)
I   0.500   0.500     0   0
R  
E     0.221

2. What is the calculated value for K? 

Back to problem questions