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In each of the following balanced oxidation–reduction equations, identify those elements that undergo changes in oxidation number and indicate the magnitude of the change in each case.

  1. I2O5 (g)+ 5 CO → I2(s) + 5CO2 (g)

  2. 2Hg2+(aq) + N2H4 (g) →2Hg (l) +N2(g) +4H+(aq)

  3. 3H2S(aq) + 2H+ (aq) + 2NO3-(aq) →3S (s) + 2NO (g) +4 H2O (l)

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Nelly Stracke
Nelly StrackeLv2
25 May 2020

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Related questions

In each of the following balanced oxidation–reduction equations, identify those elements that undergo changes in oxidation number and indicate the magnitude of the change in each case.

a)2MnO4- (aq) + 3S2-(aq) + 4H2O (l) → 3S(s) + MnO2(s) + 8OH-(aq)

b)4H2O2 (aq) + Cl2O7 (g) + 3OH-(aq) →2ClO2-(aq) + 5H2O(l) +4O2(g)

c)Ba2+(aq) +2OH-(aq) + H2O2 (aq) +2 ClO2(g) → Ba(ClO2)2(s) + 2 H2O (l) + O2(g)

Do the following balanced equations involve oxidation-reduction? If they do, identify the elements that undergo changes in oxidation number.

(a)PBr3(l) +3H2O(l)=H3PO3(aq) + 3HBr(aq)

 

(b)NaI(aq) + 3HOCl(aq)=NaIO3(aq) + HCl(aq)

 

(c)3SO2(g) + 2HNO3(aq) + 2H2O(l)=3H2SO4(aq) + 2NO(g)

 

(d) 2H2SO4(aq) + 2NaBr(s)=Br2(l) + SO2(g) + Na2SO4(aq) + 2H2O(l)

 

Indicate whether the following balanced equations involve oxidation-reduction.

If they do, identify the elements that undergo changes in oxidation number.

  1. 2AgNO3(aq) + CoCl2(aq) → 2AgCl(s) + Co(NO3)2 (aq)

  2. 2PbO2 (s) → 2 PbO(s) + O2(g)

  3. 2H2SO4(aq) + 2NaBr(s) → Br2(l) + SO2(g) + Na2SO4(aq) + 2 H2O(l)

One Class Solution:-

a) reaction is not redox

b) Pb and O change oxidation number

c) is redox reaction. S and Br change oxidation number

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