posted by BOB on .
The initial concentration for the compounds involved in the reaction displayed were determined to be [CH4(g)] = 0.9530 mol/L, [H2O(g)] = 0.9911 mol/L, [CO(g)] = 0.7474 mol/L, [H2(g)] = 0.2717 mol/L. Calculate the value of the equilibrium constant (Kc) at 1200 K if the equilibrium concentration of CO(g) was 0.8584 mol/L.
CH4(g)+H2O(g) = CO(g)+3H2(g)
i know to find Kc you have to do the products over reactants like this:
([H2]^3)([CO]) / ([CH4][H2O])
and i did the difference of 0.854 & 0.7474 for CO to get it but the answer is still not right..
the answer is 0.2561
but i keep getting 0.0158
i dono what im doing wrong..
**thanks for the help btw!!!
Your 0.0158 is not Kc because you have substituted the INITIAL concns. You are supposed to substitute equilibrium concns. I would look at this way.
........CH4 + H2O ==> ..CO +.... 3H2
So you get x by 0.8584-0.7474 = 0.1110
which allows you to find all of the other equilibrium concns. Substitute those to obtain Kc.