Question

The half-cell reactions that occur in a typical flashlight battery are: Zn(s) -t Zn2 +(aq) +2...

The half-cell reactions that occur in a typical flashlight battery are:

Zn(s) -t Zn2 +(aq) +2 e- 2

Mn02(s) + Zn2 +(aq) + 2 e- -t ZnMn204(s)

Write a chemical equation describing the net cell reaction.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

oxidation half reaction : Zn(s) ----> Zn^2+(aq) + 2 e-

reduction half reaction : 2Mn02(s) + Zn2 +(aq) + 2 e- ------> ZnMn204(s)

Zn(s) ----> Zn^2+(aq) + 2 e-

2Mn02(s) + Zn2 +(aq) + 2 e- ------> ZnMn204(s)

-----------------------------------------------------------------

2Mn02(s) + Zn(s)   ------> ZnMn204(s)

---------------------------------------------------------------

overall reaction : 2Mn02(s) + Zn(s)   ------> ZnMn204(s)

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
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.
Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e- ? Zn(s)...
Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e- ? Zn(s) E
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2...
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e‐ → Zn(s) E° = ‐ 0.76 V Al3+(aq) + 3 e‐ → Al(s) E° = ‐ 1.66 V The standard potential for the galvanic cell that uses these two half-reactions is ________ V. 2)In the galvanic cell represented by the shorthand notation shown below, Cd(aq)|Cd2+(aq)|| I2(g)|I-(aq)|Pt(s) the inert electrode is ________, and the balanced cathode half-reaction reaction is ________.
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.50molL−1 and 0.100 molL−1, respectively. Zn2+(aq)+2e−→Zn(s) E∘=−0.76V Ni2+(aq)+2e−→Ni(s) E∘=−0.23V What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.46 V?
The half-reactions that occur in ordinary alkaline batteries can be written as Cathode:MnO2(s)+H2O(l)+e−→MnO(OH)(s)+OH−(aq)Anode:Zn(s)+2OH−(aq)→Zn(OH)2(s)+2e− In 1999, researchers...
The half-reactions that occur in ordinary alkaline batteries can be written as Cathode:MnO2(s)+H2O(l)+e−→MnO(OH)(s)+OH−(aq)Anode:Zn(s)+2OH−(aq)→Zn(OH)2(s)+2e− In 1999, researchers in Israel reported a new type of alkaline battery, called a "super-iron" battery. This battery uses the same anode reaction as an ordinary alkaline battery but involves the reduction of FeO2−4 ion (from K2FeO4) to solid Fe(OH)3 at the cathode. Part A Use the following standard reduction potential and any data from Appendixes C and D to calculate the standard cell potential expected for...
What is the standard cell potential for an electrochemical cell based on the following half-reactions? IO3-(aq)...
What is the standard cell potential for an electrochemical cell based on the following half-reactions? IO3-(aq) + 6 H+(aq) + 6 e- ----> I-(aq) + 3 H2O(l ) E° = 1.085 V Zn2+(aq) + 2 e- ---> Zn(s) E° = -0.762 V
2Na+(aq)+2OH−(aq)+Zn2+(aq)+2NO3−(aq) → Zn(OH)2(s)+2Na+(aq)+2NO3−(aq) Write the net ionic equation for this precipitation reaction.
2Na+(aq)+2OH−(aq)+Zn2+(aq)+2NO3−(aq) → Zn(OH)2(s)+2Na+(aq)+2NO3−(aq) Write the net ionic equation for this precipitation reaction.
write a balanced net ionic equation for the following reaction in acidic solution: Zn(s)+VO2+(aq)->Zn2+(aq)+V3+(aq)
write a balanced net ionic equation for the following reaction in acidic solution: Zn(s)+VO2+(aq)->Zn2+(aq)+V3+(aq)
Combine the two half-reactions that give the spontaneous cell reaction with the smallest E∘. Fe2+(aq)+2e−→Fe(s) E∘=−0.45V...
Combine the two half-reactions that give the spontaneous cell reaction with the smallest E∘. Fe2+(aq)+2e−→Fe(s) E∘=−0.45V I2(s)+2e−→2I−(aq) E∘=0.54V Sn4+(aq)+2e−→Sn2+(aq) E∘=0.15V Write a balanced equation for the cell reaction. Express your answer as a chemical equation. Identify all of the phases in your answer.
3. Determine E0 Cell for the reaction: Pb2+ + Zn ---> Pb + Zn2+, the half...
3. Determine E0 Cell for the reaction: Pb2+ + Zn ---> Pb + Zn2+, the half reactions are: Pb2+ + 2e- ---> Pb E0= -0.125 Zn2+ + 2e- ---> Zn E0= -0.763 V
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT