Question

In: Chemistry

In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation...

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.


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

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

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

Solutions

Expert Solution

1)

Mn(+7)O(-2)4- + S(-2)2- + H(+1)2O(-2)                      S(0) + Mn(+4)O(-2)2 + O(-2)H(+1)-

Oxidation

S(-2)2-                             S(0)

Thus, oxidation state of Sulphur changes from -2 to 0 (Magnitude of change = 2)

Reduction

Mn(+7)O4-                     Mn(+4)O2

Oxidation state of Manganese changes from +7 to +4 (Magnitude of change = 3)

2)

H(+1)2O(-1)2 + Cl(+7)2O(-2)7 + O(-2)H(+1)-                 Cl(+3)O(-2)2- + H(+1)2O(-2) + O(0)2

Oxidation

H2O(-1)2                       O(0)2

Thus, oxidation state of Oxygen changes from -1 to 0 (Magnitude of change = 1)

Reduction

Cl(+7)2O7                   Cl(+3)O2-

Oxidation state of Chlorine changes from +7 to +3 (Magnitude of change = 4)

3)

Ba(+2)2+ + O(-2)H(+1)- + H(+1)2O(-1)2 + Cl(+4)O(-2)2              Ba(+2)(Cl(+3)O(-2)2)2 + H(+1)2O(-2) + O(0)2

Oxidation

H2O(-1)2                        O(0)2

Thus, oxidation state of Oxygen changes from -1 to 0 (Magnitude of change = 1)

Reduction

Cl(+4)O2                        Ba(Cl(+3)O2)2

Oxidation state of Chlorine changes from +4 to +3 (Magnitude of change = 1)

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation...
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 Part A 2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq) Enter your answers as chemical symbols separated by a comma. Part C 4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g) Enter your answers as chemical symbols separated by a comma Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g) Enter your answers as chemical symbols separated by a comma
Tell which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing agent,...
Tell which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. (For nonredox reactions type NONE in the answer boxes. Omit states-of-matter from your answer.) (a) Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) Is this an oxidation-reduction reaction? oxidizing agent: ? reducing agent: ? substance oxidized: ? substance reduced: ? (b) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) Is this...
For each of the following oxidation – reduction reactions, identify which element is being oxidized and...
For each of the following oxidation – reduction reactions, identify which element is being oxidized and which is being reduced? a. Ca (s) + 2H2O (l)  Ca(OH)2 (s, aq) + H2 (g) b. H2 (g) + F2 (g)  2HF (g) c. 4Fe (s) + 3O2 (g)  2Fe2O3 (s) d. 2Fe (s) + 3Cl2 (g)  2FeCl3 (s)
Using half equations for the oxidation and reduction, develop the redox equation for the oxidation of...
Using half equations for the oxidation and reduction, develop the redox equation for the oxidation of cyclohexanone under acid conditions.
Give an example of a balanced reaction with oxidation numbers for the following elements. a) selenium...
Give an example of a balanced reaction with oxidation numbers for the following elements. a) selenium b.) tellurium c.) polonium Reaction with anything. Just need an example of what that might look like.
Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair...
Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair of two half-reactions: a) H2= 2H+ + 2e- Fe2+= à Fe3+ + e- b) 1/4O2(g) + H++ e- == ½ H2OH2 =à 2H++ 2e-    C) 2IO3-+ 12H++ 10e-== I2+ 6H2O 2I-= I2+ 2e-
Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing...
Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing agent and the reducing agent. A) Cu(s) + Ag+(aq) ---> Ag(s) + Cu2+ B) Al(s) + I2(s) ---> AlI3(s) C) Pb(s) + Fe3+(aq) ----> Pb2+(aq) + Fe(s)
Write the balanced half-reactions of the following types of batteries :(oxidation and reduction both) a. Alkaline...
Write the balanced half-reactions of the following types of batteries :(oxidation and reduction both) a. Alkaline dry cell b. Nickel-Metal Hydride battery c. Zinc-air battery d. Lead storage battery
When the following oxidation–reduction reaction in a basic solution is balanced, what is the lowest whole-number...
When the following oxidation–reduction reaction in a basic solution is balanced, what is the lowest whole-number coefficient for OH−and on which side of the balanced equation should it appear? S2O82–(aq)+NO(g)→SO42–(aq)+NO3–(aq) a. 4, product side b. 8, reactant side c. 12, reactant side d. 8, product side e. 4, reactant side
Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and...
Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and label each accordingly. Give the complete balanced reaction. A.) CN-1 + MnO4-2 ---> CNO-1 + MnO2 B.) S2O3-2 + IO2-1  ---> I- + S4O6-2
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT