Here is what I would do.
Look up standard potentials for Pb to Pb^+2 and for Cr^+3 to Cr+2.
Add the reduction half to the oxidation half to obtain Ecell at standard conditions.
At standard conditions,
nFEcell = 2.303*RT*log K
F is 96,485; R is 8.314 and T is 298. Calculate K, then set up an ICE chart for the reaction and solve for the components using the K value. Check my thinking.
Lead metal is added to 0.140M Cr^+3(aq).
Pb(s)+ 2Cr^3+(aq)---> Pb^2+(aq) + 2Cr^2+(aq)
a)What is [Pb^2+] when equilibrium is established in the reaction?
b)What is [Cr^2+] when equilibrium is established in the reaction?
c)What is [Cr^3+] when equilibrium is established in the reaction?
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