Balance the following reaction using the half-reaction method in a basic solution. Clearly show each step. Clearly identify your final answer. N2(g) + NO2-(aq) à N2H4(aq) + NO3-(aq)
oxidation half reaction -------------------------------------------------reduction half reaction
NO2^-(aq) -----------> NO3^-(aq) ------------------------------------------N2(g) ----------->N2H4(aq)
NO2^-(aq)+H2O(l) -----------> NO3^-(aq) -----------------------------------N2(g) ----------->N2H4(aq)
NO2^-(aq)+H2O(l) +2OH^-(aq)-----------> NO3^-(aq) +2H2O(l)------------N2(g) +4H2O(l)----------->N2H4(aq)+ 4OH^-(aq)
NO2^-(aq)+H2O(l) +2OH^-(aq)-------> NO3^-(aq) +2H2O(l)+2e^- ---N2(g) +4H2O(l)+4e^- -------->N2H4(aq)+ 4OH^-(aq)
2NO2^-(aq)+2H2O(l) +4OH^-(aq)------> 2NO3^-(aq) +4H2O(l)+4e^-
N2(g) +4H2O(l)+4e^- ----------->N2H4(aq)+ 4OH^-(aq)
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2NO2^-(aq) + N2(g) + 2H2O(l) --------> 2NO3^- (aq) + N2H4(aq) >>>balanced equation
Balance the following reaction using the half-reaction method in a basic solution. Clearly show each step....
Show work please! Balance the following redox reaction in acidic solution using the half reaction method. Show each step clearly and show all work so that partial credit can be given if needed. 3.
PS12.1. Balance the following oxidation-reduction reactions using the half-reaction method. a) S2-(aq) + NO3-(aq) ---> S8(s) + NO2(g) acidic solution
Balance the following reaction, using the half-reaction method, in basic solution. Cr^3+ (aq) + CIO (aq) rightarrow CI_2(aq) + CrO_4^2- (aq)
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Balance the following redox reaction in basic solution by using the smallest ratio of whole number coefficients. N2H4(aq) + Cl2(g) → N2(g) + Cl–(aq) What is the coefficient for OH-(aq) in the balanced chemical equation? a 4 b 6 c 7 d 1 e 3
2. Balance the following reaction that occurs in acid, using the half-reaction method. I-1(aq) + CrO4-1(aq) --> I2(s) + Cr+3(aq) When this reaction is balanced, there will be (A) H+(aq) and (B) H2O(l) in the final balanced equation. (Enter numbers without the plus sign.) 3. Ca(NO3)2(aq) + K2CO3(aq) --> CaCO3(s) + 2 KNO3(aq) 50 mL of 1.000 M Ca(NO3)2 was reacted with excess potassium carbonate. What mass of calcium carbonate will be made? Repeat your answer to two sig figs...
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)
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3 – (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1.a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3– (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
How do I balance the following reaction in acidic conditions using the half-reaction method: As2S5 (s) + NO3- (aq) <---> H3AsO4 (aq) + HSO4- (aq) + NO2 (g) The sum of the coefficients should either be 68 or 135. Thank you.