Question

Balance each of the following by the ion-electron method. All are in acidic solution. Do not...

Balance each of the following by the ion-electron method. All are in acidic solution. Do not include states.

           

Mn2+ + BiO3¯ + H+   ____    MnO4¯ + Bi3+ + H2O

           

IO3¯ + SO2 + H2O _____ I2 + SO42¯ + H+

           

Se + BrO3¯ + H2O ________ H2SeO3 + Br¯

           

P4+ HClO + H2O ________ H3PO4 + Cl¯ + H+

           

Al + Cr2O72¯ + H+ ______ Al3+ + Cr3+ + H2O

           

ClO3¯ + I¯ + H+ _____ Cl¯ + I2 + H2O

As2O3 + NO3¯ + H2O ______ AsO43¯ + NO + H+

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Balance the following redox reaction in acidic solution using the half-reaction method, with smallest whole-number coefficients....
Balance the following redox reaction in acidic solution using the half-reaction method, with smallest whole-number coefficients. MnO4−(aq) + S2O32−(aq) → Mn2+(aq) + SO42−(aq) _____ MnO4−(aq) + _____ S2O32−(aq) + _____ H+(aq) → _____ Mn2+(aq) + _____ SO42−(aq) + _____ H2O(l)
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) O2(g) + Pb(s) → H2O(l) + Pb2+(aq) (b) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq) (c) Cl2(g) + Cr3+(aq) → Cl −(aq) + Cr2O72−(aq) (d) F2(g) + Mn2+(aq) → F −(aq) + MnO4−(aq)
Balance the following oxidation-reduction reactions on paper. Show your work. Assume all reactions occur in an...
Balance the following oxidation-reduction reactions on paper. Show your work. Assume all reactions occur in an aqueous solution. a) H2O2+Ce(SO4)2>>>Ce2(SO4)3+H2SO4+O2 b) MnCl2+NaOH+Br2>>>MnO2+NaCl+NaBr c) CrO7^-2+I^-1>>>Cr^+3+I2 (acidic) d)TeO2+BrO3^-1>>>H6TeO6+Br2 (acidic) e) N2O4+Be^-1>>>NO2^-1+BrO3^-1 (basic) f) Sb^+1+HClO>>>Sb2O5+Cl^-1 g) I2+KIO3+HCl>>>KCl+ICI h) Cl2>>>ClO3^-1+Cl^-1
1. A constant electric current flows for 3.35 h through electrolytic cells connected in series. One...
1. A constant electric current flows for 3.35 h through electrolytic cells connected in series. One contains a solution of AgNO3, and the second contains a solution of CuCl2. During this time, 1.80 g of silver is deposited in the first cell. (a) How many grams of copper are deposited in the second cell? g Cu (b) What is the current flowing in (in amperes) ?   A 2. Oxalic acid (H2C2O4) is present in many plants and vegetables. (a) Balance...
Balance each of the following redox reactions occurring in acidic solution. Part A VO2+(aq)+ClO2?(aq)?VO2+(aq)+ClO2(g) Express your...
Balance each of the following redox reactions occurring in acidic solution. Part A VO2+(aq)+ClO2?(aq)?VO2+(aq)+ClO2(g) Express your answer as a chemical equation. Identify all of the phases in your answer. Part B SO32?(aq)+MnO4?(aq)?SO42?(aq)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. Part C S2O32?(aq)+Cl2(g)?SO42?(aq)+Cl?(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT