Given the initial concentrations [H2]=[CO2]=1.65M Let x= drop in concentration o

Question

Given the initial concentrations [H2]=[CO2]=1.65M

Let x= drop in concentration of H2 ( or CO2)

The reaction is H2(g)+ CO2(g)<--->H2O(g)+CO(g)

Preparing the ICE table

Gas                                        initial concentration (M)                              Change                                Equilibrium

H2                                           1.65                                                                        -x                                            1.65-x

CO2                                        1.65                                                                        -x                                            1.65-x

H2O                                       0                                                                              x                                              x

CO                                          0                                                                              x                                              x

K= equilibrium constant = [H2O] [CO]/ [H2][CO2] = x2/(1.65-x)2= 1.6

Taking square roots, x/(1.65-x)= 1.265

Or x= 1.265*(1.65-x)

2.265x= 1.265*1.65, x= 0.92

At equilibrijm [H2] =[CO2] =1.65-x =1.65-0.92=0.73M and [H2O] =[CO2]=0.92M

Explanation / Answer

13. Calculate equilibrium concentrations: [He] = [C02-1 .65 M K =1.60 H2 + CO2= H20 (g) + CO

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