Assume that the initial concentrations of dissolved species are all 1.0M.
A) Ca(s) Cd 2 (aq) —> Ca 2 (aq) Cd(s)
B) 2Br- (aq) Sn 2 (aq) —> Br2(l) Sn(s)
C) 2Ag(s) Ni 2 (aq) —> 2Ag (aq) Ni(s)
D) Cu (aq) Fe 3 (aq) —> Cu 2 (aq) Fe 2 (aq)
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Cd is less reactive than Ca. no rxn
b. 2Br- Sn 2 –> Br2(l) Sn(s)
for this reaction to occur, Br- must be oxidized and Sn reduced
∆H decreases, ∆S decreases so ∆G will as well, i’m GUESSING that this would be spontaneous
c. Ni more reactive than Ag so rxn will take place
d. oxidation of Cu to Cu2 and reduction of Fe3 to Fe2
Cu to Cu2 = 0.3419eV
Fe3 to Fe2 = 0.771eV
Delta G = -2.303 RT log K eq.
First calculate the equilibrium constant. Then substitute in the above equation.
If Delta G is negative then the reaction is spontaneous.
If Delta G is positive then the reaction is nonspontaneous.