Question

write out the two redox half-reactions (oxidation and reduction), and use half redox half-reactions to write...

write out the two redox half-reactions (oxidation and reduction), and use half redox half-reactions to write the balanced net ionic equation of

Ag/Ag+ | | H+/H2

Cu/Cu2+ | | H+/H2

H2/H+ | | Zn2+/Zn

Cu/Cu2+ | | Zn2+/Zn

Ag/Ag+ | | Zn2+/Zn

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Oxidatio half reaction

Ag ----> Ag+ + e-

Reduction Half reaction

2H+ + 2e- ----> H2

Net ionic equation

Ag + 2H+ ------> Ag+ + H2

Oxidatio half reaction

Cu ----> Cu2+ + 2e-

Reduction Half reaction

2H+ + 2e- ----> H2

Net ionic equation

Cu + 2H+ ------> Cu2+ + H2

Oxidatio half reaction

Zn ----> Zn2+ + 2e-

Reduction Half reaction

2H+ + 2e- ----> H2

Net ionic equation

2H+ + Zn ------> Zn2+ + H2

Oxidatio half reaction

Zn ----> Zn+2 + 2e-

Reduction Half reaction

Cu2+ + 2e- ----> Cu

Net ionic equation

Zn + Cu2+ ------> Zn2+ + Cu

Oxidatio half reaction

Zn ----> Zn+2 + 2e-

Reduction Half reaction

2Ag+ + 2e- ----> Ag

Net ionic equation

Zn + 2Ag+ ------> Zn2+ + Ag

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
Write the oxidation, reduction, and redox reactions for: a) silver (Ag) reacting with Cu(NO3)2 (Why is...
Write the oxidation, reduction, and redox reactions for: a) silver (Ag) reacting with Cu(NO3)2 (Why is it that no reaction occurs here?) b) copper (Cu) reacting with Mg(NO3)2 (Why is it that no reaction occurs here?) c) zinc (Zn) reacting with Pb(NO3)2 d) lead (Pb) reacting with AgNO3 e) magnesium (Mg) reacting with NaCl (Why is it that no reaction occurs here?) Please show ALL steps and explanations. Thank you.
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The...
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The standard reduction potentials are given below. Ag+ (aq) + e- Ag (s) Eo = 0.80 V Zn2+ (aq) + 2 e- Zn(s) Eo = -0.76 V Write a balanced chemical REDOX equation and determine the Eo for the cell. What will be observed at the cathode and at the anode? Is the reaction thermodynamically favored? Explain.
For the reaction Si(s) + O2(g) --> SiO2(s): Write the balanced half cell redox reactions that...
For the reaction Si(s) + O2(g) --> SiO2(s): Write the balanced half cell redox reactions that could be used to measure the Ecell and Delta G. Label the oxidation and reduction half cell reactions
Write the balanced oxidation and reduction half reactions for reaction of Fe(II) with permanganate in acidic...
Write the balanced oxidation and reduction half reactions for reaction of Fe(II) with permanganate in acidic solution.
Identify the half reaction of oxidation and reduction in each of the following. Balance the electrons...
Identify the half reaction of oxidation and reduction in each of the following. Balance the electrons between the two reactions. Finish balancing with H+ and water Show the final reaction with the two half reactions combined Each one is worth 10 points for all work shown NO3 - +Zn→Zn2+ +NO NaCl + H2SO4 + MnO2→Na2SO4 + MnCl2 + H20 + Cl
2. Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each...
2. Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair of two half-reactions: (Show all work and steps) a)H2 →2H+ + 2e-    Fe2+ → Fe3+ + e- -------------------------------------------- b) 1/4O2 (g) + H+ + e- == ½ H2O H2 → 2H+ + 2e- -------------------------------------------- c) 2IO3- + 12H+ + 10e- == I2 + 6H2O 2I- = I2 + 2e-
(a)Two of the reactions in the “Copper Cycle” are classified as oxidation-reduction (“’redox”) reactions. Identify the...
(a)Two of the reactions in the “Copper Cycle” are classified as oxidation-reduction (“’redox”) reactions. Identify the two reactions, and identify the oxidizing agent and the reducing agent in each. (b)Which one of the redox reactions above can be classified as a single displacement reaction? (c)One of the reactions in this experiment is classified as a decomposition reaction. Identify it: (d)One of the reactions in this experiment is classified as a precipitation reaction. Identify it: (e)One of the reactions in this...
Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE...
Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE OXIDIZING AGENT in the final balanced equation: Fe2+ (aq) + MnO4- (aq) ----> Fe3+ (aq) + Mn2+ (aq)      (Acidic Solution)
8. Use the following half-reactions to write a balanced full reaction for the reduction of iron...
8. Use the following half-reactions to write a balanced full reaction for the reduction of iron (II) by copper, and compute the standard electromotive force for this reaction (spectator ions are not required). Also calculate the Gibbs energy for this reaction! Cu+ + e − → Cu E◦ = +0.52 V (1) F e2+ + 2e − → F e E◦ = −0.44 V (2)
Write the balanced net ionic equation for the following oxidation-reduction reaction occurring in acidic solution. NO2...
Write the balanced net ionic equation for the following oxidation-reduction reaction occurring in acidic solution. NO2 (g) + Cr2O72- (aq) ----> NO3- (aq) + 2Cr3+ (aq) (Please show work for the half eqautions and steps for balancing- thanks!)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT