## Chemistry and Chemical Reactivity (9th Edition)

a) Since the number of moles of reactants is equal to the number of moles of products, $K_p=K_c=56$ b) Initial concentrations: $0.045\ mol\div 10.0\ L=0.0045\ M$, reacted x $K_c=[HI]^2/[H_2][I_2]$ $56=(2x)^2/(0.0045-x)^2$ $x=0.0036\ M$ Total pressure: $P=(2\times0.0045)0.082\times698$ $P=0.515\ atm$ c) Partial pressures: $p(HI)=0.515\ atm\times(2\times0.0036)/(2\times0.0045)=0.412\ atm$ $p(H_2)=p(I_2)=0.515\ atm\times(0.0009)/(2\times0.0045)=0.052\ atm$