1. Consider the following unbalanced redox reaction: ClO4−(aq) + I−(aq) → Cl−(aq) + HIO(aq) (a) Balance...
1. Consider the following unbalanced redox reaction:
ClO4−(aq) + I−(aq) →
Cl−(aq) + HIO(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.)
ClO4−(aq) + H2O(l) + OH−(aq) + H+(aq) + e− → Cl−(aq) + H2O(l) + OH−(aq) + H+(aq) + e−
| Tries 0/3 |
I−(aq) + H2O(l)
+ OH−(aq) + H+(aq)
+ e− → HIO(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.)
ClO4−(aq) + I−(aq) + H2O(l) + OH−(aq) + H+(aq) → Cl−(aq) + HIO(aq) + H2O(l) + OH−(aq) + H+(aq)
| Tries 0/3 |
2. Consider the following unbalanced redox reaction:
NO(g) + BrO3−(aq) →
NO2−(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.)
NO(g) + H2O(l)
+ OH−(aq) + H+(aq)
+ e−
→ NO2−(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.)
NO(g) + BrO3−(aq) + H2O(l) + OH−(aq) + H+(aq) → NO2−(aq) + Br−(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.)
NO(g) + BrO3−(aq) + H2O(l) + OH−(aq) + H+(aq) → NO2−(aq) + Br−(aq) + H2O(l) + OH−(aq) + H+(aq)
Homework Answers
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1. Consider the following unbalanced redox reaction:
ClO4−(aq) + I−(aq) →
Cl−(aq) + HIO(aq)
(a) Balance...
Balance the following redox reactions by balancing the half reactions and then combine the half reactions...
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)...
2. Consider the following unbalanced redox reaction: CIO2 (aq) Cr(OH)1(s)CI(aq) +Cr04(aq) (a) Balance the corresponding half...
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....
2. Balance the following chemical reaction in basic conditions using the lowest possible whole number coefficients....
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Balance the following reaction using the lowest possible whole number coefficients, in acidic conditions. (Enter coefficients...
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 half reactions using the lowest possible whole number coefficients, in basic conditions. (Enter...
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
Balance the following half reactions using the lowest possible whole number coefficients, in acidic conditions. (Enter...
Balance the following half reactions using the lowest possible whole number coefficients, in acidic conditions. (Enter coefficients for one and zero- blanks will be marked incorrect.) 1. HIO(aq) + H+(aq) + H2O(l) + e− ⇌ I−(aq) + H+(aq) + H2O(l) + e− Tries 0/5 2. MnO4−(aq) + H+(aq) + H2O(l) + e− ⇌ Mn2+(aq) + H+(aq) + H2O(l) + e−
Balance the following half reactions using the lowest possible whole number coefficients, in basic conditions. (Enter...
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.) ClO2−(aq) + H2O(l) + OH−(aq) + e− ⇌ Cl−(aq) + H2O(l) + OH−(aq) + e− MnO42−(aq) + H2O(l) + OH−(aq) + e− ⇌ MnO2(s) + H2O(l) + OH−(aq) + e−
Balance the redox reactions: basic: ClO-(aq)+Cr(OH)4-(aq)----> CrO42-(aq)+Cl-(aq) MnO4-(aq)+Br-(aq)--> MnO2(s)+BrO3-(aq) NO2-(aq)+Al(s)--->NH3(g)+AlO2- Aidic: ClO4-(aq)+Cr(OH)4---->ClO3-(aq)+Cl2(g)
Balance the redox reactions: basic: ClO-(aq)+Cr(OH)4-(aq)----> CrO42-(aq)+Cl-(aq) MnO4-(aq)+Br-(aq)--> MnO2(s)+BrO3-(aq) NO2-(aq)+Al(s)--->NH3(g)+AlO2- Aidic: ClO4-(aq)+Cr(OH)4---->ClO3-(aq)+Cl2(g)
In acidic solution, bromate ion can be used to react with a number of metal ions....
In acidic solution, bromate ion can be used to react with a number of metal ions. One such reaction is: BrO3−(aq)+Sn2+(aq)→Br−(aq)+Sn4+(aq). Since this reaction takes place in acidic solution, H2O(l) and H+(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:BrO3−(aq)+Sn2+(aq)+−→Br−(aq)+Sn4+(aq)+ −−−AWhat are the coefficients of the six species in the balanced equation above? Remember to include coefficients for H2O(l) and H+(aq) in the appropriate blanks. B)What are...
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons...
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...
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....
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