Balancing Oxidation–Reduction Reactions (Section)
Complete and balance the following equations, and identify the oxidizing and reducing agents:
(a) Cr2O72-(aq) + I-(aq)→Cr3+(aq) + IO3-(aq) (acidic solution)
(b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) +HCO2H(aq) (acidic solution)
(c) I2(s) + OCl-(aq)→IO3-(aq) + Cl-(aq) (acidic solution)
(d) As2O3(s) + NO3-(aq)→H3AsO4(aq) + N2O3(aq) (acidic solution)
(e) MnO4-(aq) + Br-(aq)→MnO2(s) + BrO3-(aq) (basic solution)
(f) Pb(OH)42-(aq) + ClO-(aq)→PbO2(s) + Cl-(aq) (basic solution)
(a)
Two half cell reactions
To balance the number of o-atoms by adding
To balance the number of H-atoms by adding
To balance the charge
Overall equation: -
By adding the above equation
(b)
Two half cell reactions
To balance the number of O-atoms by adding
To balance the number of H-atom by adding
To balance the charge: -
Multiplied equation (1) by 4 and (2) by 5
Overall equation by adding both of them
Change in oxidation state of
is an oxidizing agent as it is reduced thus is a reducing agent.
(c)
Two half cell reactions
To balance the number of O-atom by adding
To balance the number of H-atoms by adding
To balance the charge
Multiplied equation (2) by 5
Overall reaction by adding both the equation
Change in oxidation state of I and C1.
is oxidized thus it’s a reducing agent and is an oxidizing agent.
(d)
Two half cell reactions
To balance the number of O-atom by adding
To balance the number of H-atom by adding
To balance the charge: -
Overall reaction by adding the two reactions
Change in oxidation state of.
is oxidized thus it’s a reducing agent and is an oxidizing agent.
(e)
Two half cell reactions
To balance the number of O-atoms by adding
To balance the number of H-atoms by adding
To balance the charge: -
Multiplied equation and added to both sides of
the reaction
Overall reaction-:
Change in oxidation state of .
is reduced thus its an oxidizing agent and is the reducing agent.
(f)
Two half cell reactions
To balance the number of O-atom by adding
To balance the number of H-atom by adding-:
To balance the charge-:
Added the two equations: -
To neutralize ion, added to both sides-:
To determine the change in oxidation state-:
is oxidized thus it’s a reducing agent and is an oxidizing agent.
Balancing Oxidation–Reduction Reactions (Section)Complete and balance the following equations, and identify the oxidizing and reducing agents:(a)...
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) NO3- (aq) + As2O3(s) = N2O3(aq) + H3ASO4(aq) N03* + As2O3 + H+ + O H20=O N203+ H3A504 + H+ + H20 (b) Clozaq) + As(s) Æ HClO(aq) + H3AsO3(aq) DC103+ As + OH+ + H2O=OHCO + H2A503 + H+ + OH20 (c) CIO-(aq) + Pb(OH)42-(aq) = Cl(aq) + PbO2(s) D clo + Pb(OH)42- + D OH + H2O=D C + PbO2 + OH +...
How do I solve the following redox reactions? What are the balanced half-reactions? What is the final balanced equation? Problems 1. MnO4 (aq) + SO32- (aq) → MnO2 (s) + SO42- (aq) in basic solution 2. NO2" (aq) + Al(s) NH3(aq) + Al(OH)4 (aq) in basic solution 3. Mn2+ (aq) + NaBiO3 (s) → Bi* (aq) + MnO4 (aq) + Nat (aq) in acidic solution 4. As2O3 (s) + NO3- (aq) → H3ASO4 (aq) + N2O3 (aq) in acidic solution...
Balance the following redox reactions: a) CN− + MnO4− → CNO− + MnO2 (basic solution) b) O2 + As → HAsO2 + H2O (acidic solution) c) Br− + MnO4− → MnO2 + BrO3− (basic solution) d) NO2 → NO3− + NO (acidic solution) e) ClO4− + Cl− → ClO− + Cl2 (acidic solution) f) AlH4− + H2CO → Al3+ + CH3OH (basic solution)
More Practice Balancing Redox Reactions in Acid and Basic Solution Balance the following redox reaction in both acidic and basic solution using the half reaction method outlined in Recitation 10, Part III. 3. Unbalanced: PbO2(s) + Mn2+(aq) → Pb2+ (aq) + MnO4- (aq) 4. Unbalanced: SO42-(aq) + Cr3+(aq) → SO2(g) + Cr2O72-(aq)
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 + H2O (in basic solution) (b) Bi(OH)3 + SnO22− → SnO32− + Bi (in basic solution) (c) Cr2O72− + C2O42− → Cr3+ + CO2 (in acidic solution) (d) ClO3− + Cl− → Cl2 + ClO2 (in acidic solution) (e) Mn2+ + BiO3− → Bi3+ + MnO4− (in acidic solution)
1. 1. Balance the following skeleton reactions and identify the oxidizing and reducing agents: (a) Mn+ (aq) + BiO3 (aq) →MnO4 (aq) + Bit (aq) (acidic) (b) Fe(OH)2(s) + Pb(OH)3 (aq) Fe(OH)3(s) + Pb(s) (basic)
7. Balance the following equations using the oxidation number method. Identify the oxidizing and reducing agents. In basic solution: _MnO4 (aq) +_ CIO (aq) → _MnO2 (s) +_ CIO. (aq) In acidic solution: KCIO3(aq) + _Br" (aq) → __KCI (aq) + ___ Br2 (aq)
[15] Balance the following redox reactions: {3 points each} a) Cr2O72-(aq) + Cl-(aq) → Cr3+(aq) + Cl2(g) (acidic medium) b) Al(s) + MnO4-(aq) → MnO2(s) + Al(OH)4-(aq) (basic medium)
Balance the following redox reactions by balancing the half reactions and then combine the half reactions to get the overall balanced redox reaction with the lowest possible whole number coefficients. 1. Consider the following unbalanced redox reaction: MnO2(s) + BrO3−(aq) → MnO4−(aq) + Br−(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) MnO2(s) + H2O(l) + OH−(aq) + H+(aq) + e− → MnO4−(aq) + H2O(l) + OH−(aq) + H+(aq)...
5) Balance the following redox reactions. For each one, identify the reducin and the oxidizing agent. (acidic solution) a) Cr2O72- + NO2 = Cr3+ + NO3- (basic solution) b) H O2 + Cio2 = 02 + ClO2- (acidic solution) c) Mnox + VÕ2+ = Mn2+ + V(OH)4* d) AIS) + Noz = NH4+ + A102 (basic solution) e) 103- + 1 = 12 (acidic solution) f) SCN-+ Br03- = Br + SO42- + HCN (acidic solution)