Explore BrainMass
Share

Electrochemistry: Spontaneity of Redox Reactions

This content was STOLEN from BrainMass.com - View the original, and get the already-completed solution here!

I need help with the following problem with steps included:

What is the equilibrium constant for the following reaction at 25oC?

Mg(s) + Zn2+(aq)ï?  Mg2+(aq) + Zn(s)

I have also attached the problem in its correct form if you need to see the correct format

© BrainMass Inc. brainmass.com October 17, 2018, 1:01 am ad1c9bdddf
https://brainmass.com/chemistry/redox-reactions/electrochemistry-spontaneity-of-redox-reactions-320748

Attachments

Solution Preview

19.21 What is the equilibrium constant for the following reaction at 25oC?
Mg(s) + Zn2+(aq) Mg2+(aq) ...

Solution Summary

The solution is comprised of an explanation on how to balance a redox reaction.

$2.19
Similar Posting

Electrochemistry- Cathodes and Anodes

(there are six procedures with the same questions for each procedure)

Procedure 1 LAB:

Beaker #1: 150 ml CuSO4
Beaker #2: 150 ml SnCl2
Salt Bridge connects the two beakers
electrode in CuSO4 is set to copper
electrode in SnCl2 is set to tin
volt meter reads .4761

Question:

1. Identify the cathode and anode in this system.

2. Use the table for Standard Reduction Potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does teh calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

Procedure 2 LAB:

Beaker #1 150 ml CuSO4
Beaker #2 150 ml AgNO3
Salt bridge connects the two
electrode for beaker #1 set to copper
electrode for beaker #2 set to silver
Volt meter reads -.4594

Questions

1. Identify the cathode and anode in this system.

2. Use the table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell sy about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

LAB Procedure 3

Beaker #1 150 ml CuSO4
Beaker #2 150 ml ZnSO4
Salt Bridge
electrode CuSO4 set to copper
electrode ZnSO4 set to zinc
Volt meter reads 1.103

Questions

1. Identify the cathode and anode in this system.

2. Use table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

Procedure 4 LAB

Beaker #1 150ml SnCl2
Beaker #2 150ml ZnSO4
Salt bridge
electrode SnCl2 set to tin
electrode ZnSO4 set to zinc
Volt meter reads .6269

Questions

1. Identify the cathode and anode in this system.

2. Use the table for standard reduction potentials at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell say about the spontaneity of this redox reduction? Are products or reactants favored? How do you know?

Procedure 5 LAB

Beaker #1 150ml SnCl2
Beaker #2 150ml AgNO3
Salt Bridge
electrode SnCl2 set to tin
electrode AgNO3 set to silver
Volt meter reads -.9357

Questions

1. Identify the cathode and anode in this system.

2. Use the table for standard reduction potential at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are the products or reactants favored? How do you know?

Procedure 6 LAB

Beaker #1 150ml ZnSO4
Beaker #2 150ml AgNO3
Salt bridge
electrode ZnSO4 set to zinc
electrode AgNO3 set to silver
Volt meter reads -1.562

Question

1. Identify the cathode and anode in this system.

2.Use the table for standard reduction potential at 25 degrees C (half reaction table increasing strength as an oxidizing agent). How does the calculated value compare to the experimentally obtained value?

3. What does the reduction potential of this cell say about the spontaneity of this redox reaction? Are products or reactants favored? How do you know?

View Full Posting Details