3) The list below shows the reduction potentials for ten different metal ions. (

Question

3) The list below shows the reduction potentials for ten different metal ions. (a) Calculate AE for the redox reaction: Ni(s) +Mn2 (aq)- Ni(aq)+Mn(s) Will this reaction occur spontaneously? (b) Calculate AB for the redox reaction: Co(s)+Sn2+(a) Co+(aq)+Sn(s) Will this reaction occur spontaneously? Half-Reaction E(V) Cu (aq)+2e Cu(s) +0.34 Pb (aq) +2e-Pb(s) -0.13 Sn2+(aq) + 2e-? Sn(s) -0.14 Ni2(aq) +2e-Ni(s) -0.25 Co (aq) +2eCo(s) 0.28 Cd* (aq) + 2e Cd(s) -0.40 Fe2+(aq) + 2e-? Fe(s) -0.44 Zn2(aq) + 2e>Zn(s) -0.76 Mn2(aq) + 2eMn(s) -1.18 Mg (aq) + 2e Mg(s) -2.37

Explanation / Answer

3) The more the value of Eo cell , the greater the force for the electrons through the system, thus the reaction is more spontaneous

a) Ni + Mn2+ ------> Ni2+ + Mn

delta Erxn = sum of delta E of products - sum of the delta E of reactants
                = [Ni2+ + Mn ] - [ Ni + Mn2+ ]
               = [Ni2+ - Ni ] + [ Mn - Mn2+ ] = - (-0.25) + (-1.18) = - 0.93 V
Reaction is not spontaneous

b) Co + Sn2+ -------> Co2+ + Sn
delta Erxn = sum of delta E of products - sum of the delta E of reactants
                  = [ Co2+ + Sn ] - [ Co + Sn2+ ]
                 = [ Co2+ - Co ] + [Sn - Sn2+ ] = -(-0.28) + (-0.14) = + 0.14 V
Reaction is Spontaneous

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