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jeka94
3 years ago
8

Balance each of the following in BASE: Show work

Chemistry
1 answer:
kupik [55]3 years ago
7 0

Answer : The balanced chemical equation in a basic solution are,

(A) 2CrO_4^{2-}+8H_2O+3Cu\rightarrow 2Cr(OH)_3+4OH^-+3Cu(OH)_2

(B) 2NO_2+2OH^-\rightarrow NO_3^-+H_2O+NO_2^-

(C) 4Zn+7OH^-+NO_3^-+6H_2O\rightarrow 4[Zn(OH)_4]^{2-}+NH_3

(D) Br_2+12OH^-+5Br_2\rightarrow 2BrO_3^-+6H_2O+10Br^-

Explanation :

<u>(A) The given chemical reaction is :</u>

CrO_4^{2-}(aq)+Cu(s)\rightarrow Cr(OH)_3(s)+Cu(OH)_2(s)

The oxidation-reduction half reaction will be :

Oxidation : Cu\rightarrow Cu^{2+}+2e^-

Reduction : CrO_4^{2-}+4H_2O+3e^-\rightarrow Cr^{3+}+8OH^-

In order to balance the electrons, we multiply the oxidation reaction by 3 and reduction reaction by 2 then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

2CrO_4^{2-}+8H_2O+3Cu\rightarrow 2Cr^{3+}+16OH^-+3Cu^{2+}

or,

2CrO_4^{2-}+8H_2O+3Cu\rightarrow 2Cr(OH)_3+4OH^-+3Cu(OH)_2

<u>(B) The given chemical reaction is :</u>

NO_2(g)\rightarrow NO_3^-(aq)+NO_2^-(aq)

The oxidation-reduction half reaction will be :

Oxidation : NO_2+2OH^-\rightarrow NO_3^-+H_2O+1e^-

Reduction : NO_2+1e^-\rightarrow NO_2^-

The electrons in both the reactions are balanced. Now added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

2NO_2+2OH^-\rightarrow NO_3^-+H_2O+NO_2^-

<u>(C) The given chemical reaction is :</u>

Zn(s)+NO_3^-(aq)\rightarrow Zn(OH)_4^{2-}(aq)+NH_3(g)

The oxidation-reduction half reaction will be :

Oxidation : Zn+4OH^-\rightarrow [Zn(OH)_4]^{2-}+2e^-

Reduction : NO_3^-+6H_2O+8e^-\rightarrow NH_3+9OH^-

In order to balance the electrons, we multiply the oxidation reaction by 4 and then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

4Zn+7OH^-+NO_3^-+6H_2O\rightarrow 4[Zn(OH)_4]^{2-}+NH_3

<u>(D) The given chemical reaction is :</u>

Br_2(l)\rightarrow BrO_3^-(aq)+Br^-(aq)

The oxidation-reduction half reaction will be :

Oxidation : Br_2+12OH^-\rightarrow 2BrO_3^-+6H_2O+10e^-

Reduction : Br_2+2e^-\rightarrow 2Br^-

In order to balance the electrons, we multiply the reduction reaction by 5 and then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

Br_2+12OH^-+5Br_2\rightarrow 2BrO_3^-+6H_2O+10Br^-

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