Consider the following equations for a cell reaction, A + B rarr C + D , E^(@) = x "volt", Delta G= Delta G_(1) 2A + 2B rarr 2C + 2D, E^(@) = y "volt", DeltaG = DeltaG_(2) Then,
In the following equilibria I:A+2B hArr C, K_(eq)=K_(1) II: C+DhArr 3A, K_(eq)=K_(2) III, 6B+D hArr 2C, K_(eq)=K_(3) Hence,
Calculate the half-cell potential at 298 K for the reaction, Zn^(2+)+2e^(-) rarr Zn If [Zn^(2+)]=0.1 M and E^(@)=-0.76 volt.
For the reactions A hArr B, K_(c ) =1 B hArr C, K_(c)=2 C hArr D, K_(c)=3 K_(c) for the reaction A hArr D is
What is the K_(eq) expression for the reaction, C(s)+CO_2(g)to2CO(g) ?