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Identify the elements that undergo changes in oxidation number in the reactions:


•NaI(aq)+3HOCl(aq)→NaIO3(aq)+3HCl(aq)


___________

3SO2(g)+2HNO3(aq)+2H2O(l)→3H2SO4(aq)+

2NO(g)

________

•2H2SO4(aq)+2NaBr(s)→Br2(l)+SO2(g)+

Na2SO4(aq)+2H2O(l)

Verified Answer :

MissPhiladelphia

The first reaction is
•NaI(aq)+3HOCl(aq)→NaIO3(aq)+3HCl(aq)

The elements that undergo changes in oxidation number are Iodine and Chlorine

The second reaction is
3SO2(g)+2HNO3(aq)+2H2O(l)→3H2SO4(aq)+2NO(g)

The elements that undergo changes in oxidation number are Sulfur and Nitrogen

The third reaction is
•2H2SO4(aq)+2NaBr(s)→Br2(l)+SO2(g)+Na2SO4(aq)+2H2O(l)

The elements that undergo changes in oxidation number are Sulfur and Bromine

Explanation:

1) \(NaI(aq)+3HOCl(aq)\rightarrow NaIO_3(aq)+3HCl(aq)\)

The iodine elements is going under oxidation in the given reaction that is from -1 to +5.

NaI

1+x=0

x=-1

In NaI , the oxidation state of iodine is -1

1+x+(3)(-2)=0

x = +5

In \(NaIO_3\) , the oxidation state of iodine is +5.

2) \(3SO_2(g)+2HNO_3(aq)+2H_2O(l)\rightarrow 3H_2SO_4(aq)+2NO(g)\)

The sulfur elements is going under oxidation in the given reaction ythat is from +4 to +6.

\(SO_2\)

x+(2)(-2)=0

x = +4

In\(SO_2\) , the oxidation state of sulfur is +4.

\(H_2SO_4\)

2+x+(4)(-2)=0

x = +6

In \(H_2SO_4\) , the oxidation state of sulfur is +6.

3)\(2H_2SO_4(aq)+2NaBr(s)\rightarrow Br_2(l)+SO_2(g)+Na_2SO_4(aq)+2H_2O(l)\)

The bromine elements is going under oxidation in the given reaction that is from -1 to 0.

NaBr

1+x=0

x=-1

in NaBr the oxidation state of bromine is -1.

\(Br_2\)

2(x)=0

x = 0

In \(Br_2\) , the oxidation state of bromine is 0.

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