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Balance the following redox reaction. If you have 1.0 mols of each reactant, what is the...


Balance the following redox reaction. If you have 1.0 mols of each reactant, what is the limiting reagent?

ClO-(aq) + H+(aq) + Cu(s) → Cl-(aq) + H2O(l) + Cu2+(aq)

Solutions

Expert Solution

ClO-(aq) + H+(aq) + Cu(s) → Cl-(aq) + H2O(l) + Cu2+(aq)

O.H.R                                                                     R.H. R

Cu(s) ------> Cu^2+(aq)                         ClO^- (aq) ------------------> Cl^- (aq)

Cu(s) ------> Cu^2+(aq)                         ClO^- (aq) ------------------> Cl^- (aq) + H2O

Cu(s) ------> Cu^2+(aq)                         ClO^- (aq) +2H^+ (aq)------------------> Cl^- (aq) + H2O

Cu(s) ------> Cu^2+(aq) +2e^-            ClO^- (aq) +2H^+ (aq)+2e^- ------------> Cl^- (aq) + H2O

                  Cu(s) ------> Cu^2+(aq) +2e^-           

            ClO^- (aq) +2H^+ (aq)+2e^- ------------> Cl^- (aq) + H2O

----------------------------------------------------------------------------------------------

ClO-(aq) + 2H+(aq) + Cu(s) → Cl-(aq) + H2O(l) + Cu2+(aq)

1 mole of ClO^- produce 1 mole of H2O

1 mole of ClO^- produce 1 mole of H2O

2 mole of H^+ produced 1 mole of H2O

1 mole of H^+ produced = 1*1/2 = 0.5 moles of H2O.

H^+ is limiting reagent >>>>answer

queen_honey_blossom answered 2 years ago
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