Balance the half-reactions assuming that they occur in acidic solution.Express your answer as a balanced half-reaction....

Balance the half-reactions assuming that they occur in acidic solution.Express your answer as a balanced half-reaction. Identify all of the phases in your answer.

1) NO3−(aq)→NO(g)

2)Zn(s)→Zn2+(aq)

3)Te(s)→TeO2(s)

4)Sn4+(aq)→Sn2+(aq)

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

3. Balance the following redox reactions that occur in acidic solution using the half-reaction method. a....

3. Balance the following redox reactions that occur in acidic solution using the half-reaction method. a. Cr(s) + NO3-(aq) → Cr3+(aq) + NO(g) b. CH3OH(aq) + Ce4+(aq) → CO2(aq) + Ce3+(aq) c. SO32-(aq) + MnO4-(aq) → SO42-(aq) + Mn2+(aq)

6. Write balanced redox half reactions (assuming acidic conditions) for the conversion of: a. ammonium to...

6. Write balanced redox half reactions (assuming acidic conditions) for the conversion of: a. ammonium to nitrate b. nitrite to nitrogen gas.

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

Balance the following redox reactions, in base, using the half-reaction method. Clearly identify each balanced half-reaction...

Balance the following redox reactions, in base, using the half-reaction method. Clearly identify each balanced half-reaction and the overall balanced equation. C3H8O2 (a) + Cr2O72– (aq)  C3H4O4 (aq) + 2 Cr3+ (aq)

Complete and Balance the following half-reactions (steps2-5 in half reaction method): MnO4−(aq) ⟶ Mn2+(aq) (in acidic...

Complete and Balance the following half-reactions (steps2-5 in half reaction method): MnO4−(aq) ⟶ Mn2+(aq) (in acidic solution)

1. a) Show the balanced half reactions and the total balanced reaction for the following redox...

1. a) Show the balanced half reactions and the total balanced reaction for the following redox reaction in acidic solution. RuO4 + H2SeO3 → Ru3+ + SeO42- b) Comment on whether you expect this reaction to be spontaneous. Show all of your work.b 2 (a) Use the Lattimer diagram for chlorine in basic conditions to determine the potential for reduction of ClO4- to Cl2 . (b) Write a balanced equation for this half reaction

Write the balanced overall reaction from these unbalanced half-reactions

Balance each of the following half-reactions, assuming that they occur in basic solution. CH3OH(aq)?CH2O(aq)

4. Balance the following redox reactions that occur in basic solution using the half-reaction method. a....

4. Balance the following redox reactions that occur in basic solution using the half-reaction method. a. PO33-(aq) + MnO4-(aq) → PO43-(aq) + MnO2(s) b. Mg(s) + OCl-(aq) → Mg(OH)2(s) + Cl-(aq) c. H2CO(aq) + Ag(NH3)2+(aq) → HCO3-(aq) + Ag(s) + NH3(aq)

1. Write the balanced oxidation and reduction half reactions for the reaction of (As_2O_3)^3- and I_2....

1. Write the balanced oxidation and reduction half reactions for the reaction of (As_2O_3)^3- and I_2. What ion is oxidized and what ion is reduced? 2. Assuming that 5 mL of 0.006M arsenite solution is subjected to coulometric titration using a current of 30 mamps. Calculate the time that the current should be applied to reach the endpoint of the titration.

Subjects