Question

What is the calculated value of the cell potential at 298K for an electrochemical cell with...

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 1.44 M and the Mg2+ concentration is 1.47×10-4 M ?

Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)

Answer:  V

The cell reaction as written above is spontaneous for the concentrations given:
_______
true
false

Homework Answers

Answer #1


Lets find Eo 1st
from data table:
Eo(Mg2+/Mg(s)) = -2.372 V
Eo(Cu2+/Cu(s)) = 0.337 V

As per given reaction/cell notation,
cathode is (Cu2+/Cu(s))
anode is (Mg2+/Mg(s))

Eocell = Eocathode - Eoanode
= (0.337) - (-2.372)
= 2.709 V

Number of electron being transferred in balanced reaction is 2
So, n = 2

use:
E = Eo - (2.303*RT/nF) log {[Mg2+]^1/[Cu2+]^1}

Here:
2.303*R*T/F
= 2.303*8.314*298.0/96500
= 0.0591

So, above expression becomes:
E = Eo - (0.0591/n) log {[Mg2+]/[Cu2+]}
E = 2.709 - (0.0591/2) log ((1.47*10^-4)/1.44)
E = 2.709-(-0.118)
E = 2.827 V
Answer: 2.83 V

Since E is positive, this is spontaneous
Answer: True

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 7.38×10-4 M and the Al3+ concentration is 1.43 M ? 3Cu2+(aq) + 2Al(s)3Cu(s) + 2Al3+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: True or False?
A) What is the calculated value of the cell potential at 298K for an electrochemical cell...
A) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 8.15×10-4 atm, the Cl- concentration is 1.48M, and the Pb2+ concentration is 1.07M ? Cl2(g) + Pb(s) ---> 2Cl-(aq) + Pb2+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given:____ ( TRUE/FALSE ) B)What is the calculated value of the cell potential at 298K for an electrochemical cell with...
1. What is the calculated value of the cell potential at 298K for an electrochemical cell...
1. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 4.09×10-4 M and the Mg2+ concentration is 1.03 M ? Pb2+(aq) + Mg(s) ---> Pb(s) + Mg2+(aq) Answer: ___V The cell reaction as written above is spontaneous for the concentrations given____. (true or false) (From the table of standard reduction potentials: ) Pb2+(aq) + 2 e- --> Pb(s) -0.126 Mg2+(aq) + 2 e- --> Mg(s)...
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 1.23 M and the Cr3+ concentration is 5.82×10-4 M ? 3Cu2+(aq) + 2Cr(s)-->3Cu(s) + 2Cr3+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 1.20 M and the Mn2+ concentration is 5.43×10-4 M ? Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq) Answer: in V The cell reaction as written above is spontaneous for the concentrations given: true or false?
When the Cu2+ concentration is 1.40 M, the observed cell potential at 298K for an electrochemical...
When the Cu2+ concentration is 1.40 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.805V. What is the Mg2+ concentration? Cu2+(aq) + Mg(s) -----> Cu(s) + Mg2+(aq) Answer: ______M
What is the calculated value of the cell potential at 298 K for an electrochemical cell...
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 5.00×10-3 bar, the H+ concentration is 1.46 M, and the Zn2+concentration is 3.42×10-4 M ? 2H+(aq) + Zn(s) ----> H2(g) + Zn2+(aq) Answer: _____ V ? The cell reaction as written above is product-favored (spontaneous) for the concentrations given: _______(true/false)?
A) When the Cu2+ concentration is 1.07 M, the observed cell potential at 298K for an...
A) When the Cu2+ concentration is 1.07 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.607V. What is the Mn2+ concentration? Cu2+(aq) + Mn(s)--> Cu(s) + Mn2+(aq) Answer: _____ M B) When the Cu2+ concentration is 5.71×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.609V. What is the Mg2+ concentration? Cu2+(aq) + Mg(s)---> Cu(s) + Mg2+(aq) Answer: _____ M C) When the Cu2+...
When [ Pb2+] = 1.00 M, the observed cell potential at 298K for an electrochemical cell...
When [ Pb2+] = 1.00 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 1.611 V. What is the Al3+concentration in this cell? 3 Pb2+(aq) + 2 Al (s) ----> 3 Pb (s) + 2 Al3+(aq) [ Al3+] = ______M
Given a potential of 0.456 V, for the following electrochemical cell, what is the concentration of...
Given a potential of 0.456 V, for the following electrochemical cell, what is the concentration of Ag+? Cu2+(aq) (1.0 M)|Cu(s)||Ag+(aq)|Ag(s)