## Chemistry and Chemical Reactivity (9th Edition)

a) Initial concentration: $0.50\ mol\div 9.50\ L=0.0526\ M$, reacted x: $K=[CO][Br_2]/[COBr_2]$ $0.190=x\times x/(0.0526-x)$ $x^2+0.190x-0.01=0$ $x=0.043$ $[CO]=[Br_2]=0.043\ M,[COBr_2]=0.01\ M$ b) Initial concentration: $0.50\ mol\div 4.50\ L=0.111\ M$, reacted x: $K=[CO][Br_2]/[COBr_2]$ $0.190=x\times x/(0.111-x)$ $x^2+0.190x-0.021=0$ $x=0.078$ $[CO]=[Br_2]=0.078\ M,[COBr_2]=0.033\ M$ c) The equilibrium shifted to the left, since $0.033\ M\times4.5\ L>0.01\ M\times9.5\ L$