What is the balanced equation when aluminum reacts with copper (ii) sulfate? i don't know how to do this
1 answer:
Here Cu (II) reduced to Cu (0). Al would be strong reducing agent to do so. Now ... Compare Al and Cu reduction potentials. Al3+(aq) + 3 e– ----> Al(s) -1.66
Cu(OH)2(s) + 2 e– ----> Cu(s) + 2 OH–(aq) -0.36. It implies that reduction potential of Cu is more than Al hence this reaction is not feasible bcuz copper is a reducing agent ( oxidize itself or reduces others). But still you can balance...practically this reaction seems impossible bcuz of above reason.
Cu(OH)2(s) + 2 e– ----> Cu(s) + 2 OH–(aq) -0.36. It implies that reduction potential of Cu is more than Al hence this reaction is not feasible bcuz copper is a reducing agent ( oxidize itself or reduces others). But still you can balance...practically this reaction seems impossible bcuz of above reason.
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We have a solution of NaOH and H₂CO₃
First, NaOH will dissociate into Na⁺ and OH⁻ ions
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The H⁺ released from the substitution will bond with the OH⁻ ion to form a water molecule
If there were to be another NaOH molecule, a similar substitution will take place, substituting the second hydrogen from H₂CO₃ as well to form Na₂CO₃
