## Chemistry and Chemical Reactivity (9th Edition)

a) The concentrations of CO and H2O are $0.11\ mol\div 50.0\ L=0.0022\ M$, and of H2 and CO2 are $0.087\ mol\div 50.0\ L=0.00174\ M$. The equilibrium constant is given by: $K=[CO][H_2O]/[CO_2][H_2]$ $K=0.0022\times0.0022/0.0017/0.0017=1.60$ b) Number of moles reacted of CO2 and H2 each: x Number of moles of H2O and CO formed: x $K=[CO][H_2O]/[CO_2][H_2]$ $K=(x/V).(x/V)/[(0.010-x)/V(0.010-x)/V]$ $1.60=x^2/(0.010-x)^2$ $1.265\times(0.010-x)=x$ $x=0.0056$ 0.0056 mol of each