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) + e−
Tries 0/3 |
BrO3−(aq) + H2O(l)
+ OH−(aq) + H+(aq)
+ e− → Br−(aq)
+ H2O(l) + OH−(aq)
+ H+(aq) + e−
Tries 0/3 |
(b) Using the results from part (a), balance the full reaction
in acidic conditions with the lowest possible
whole number coefficients.
(Enter coefficients for one and zero. Blanks will be marked
incorrect.)
MnO2(s) + BrO3−(aq) + H2O(l) + OH−(aq) + H+(aq) → MnO4−(aq) + Br−(aq) + H2O(l) + OH−(aq) + H+(aq)
Tries 0/3 |
2. Consider the following unbalanced redox reaction:
AsO2−(aq) + ClO−(aq) → As(s) +
ClO2−(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.)
AsO2−(aq) + H2O(l)
+ OH−(aq) + H+(aq)
+ e− → As(s)
+ H2O(l) + OH−(aq)
+ H+(aq) + e−
Tries 0/3 |
ClO−(aq) + H2O(l)
+ OH−(aq) + H+(aq)
+ e−
→ ClO2−(aq)
+ H2O(l) + OH−(aq)
+ H+(aq) + e−
Tries 0/3 |
(b) Using the results from part (a), balance the full reaction
in acidic conditions with the lowest possible
whole number coefficients.
(Enter coefficients for one and zero. Blanks will be marked
incorrect.)
AsO2−(aq) + ClO−(aq) + H2O(l) + OH−(aq) + H+(aq) → As(s) + ClO2−(aq) + H2O(l) + OH−(aq) + H+(aq)
Tries 0/3 |
(c) Using the results from part (b), balance the full reaction
in basic conditions with the lowest possible whole
number coefficients.
(Enter coefficients for one and zero. Blanks will be marked
incorrect.)
AsO2−(aq) + ClO−(aq) + H2O(l) + OH−(aq) + H+(aq) → As(s) + ClO2−(aq) + H2O(l) + OH−(aq) + H+(aq)
Balance the following redox reactions by balancing the half reactions and then combine the half reactions...
Balance the following half reactions using the lowest possible whole number coefficients, in basic conditions. (Enter coefficients for one and zero- blanks will be marked incorrect.) 1. Br−(aq) + H2O(l) + OH−(aq) + e− ⇌ BrO3−(aq) + H2O(l) + OH−(l) + e− Tries 0/5 2. AgO(s) + H2O(l) + OH−(aq) + e− ⇌ Ag2O3(s) + H2O(l) + OH−(l) + e− Tries 0/5
2. Consider the following unbalanced redox reaction: CIO2 (aq) Cr(OH)1(s)CI(aq) +Cr04(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients Enter coeffcients for one and zero. Blanks i be marked incorrect.) CIO2 (aq) + Submil Answer Tries 0/3 H20(I) + OH (aq) + Submi AnserTries 0/3 (b) Using the results from part (a), balance the full reaction in acidic conditions with the lowest possible whole number coefficients. (Enter coefficients for one and zero....
Balance the following reaction using the lowest possible whole number coefficients, in acidic conditions. (Enter coefficients for one and zero- blanks will be marked incorrect.) HBrO(aq) + HAsO2(aq) + H+(aq) + H2O(l) + OH−(aq) → Br−(aq) + H3AsO4(aq) + H+(aq) + H2O(l) + OH−(aq)
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)
Balancing RedOx Reactions in Acidic or Basic Aqueous Solution Read: Section 4.11, Zumdahl, "Chemical Principles" 8th ed. Compare ⇒ A worked example using the oxidation number method. Compose the balanced reaction equation for the following reaction occuring in acidic aqueous medium. Reduce all coefficients to the lowest possible integers. Hg(l) + NO3−(aq) → Hg22+(aq) + NO(g) Select the coefficients below, (appropriately including or excluding H2O(l) and H+(aq)). NO3−(aq) + Hg(l) + H+(aq) + H2O(l) → NO(g) + Hg22+(aq) + H+(aq)...
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method H2O(l), OH−(aq), and H+(aq) may be added to complete the mass balance. Which...
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 +...
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
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)
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)