For the reaction 2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl2 (g). E=0.483 V what is the cell potential at 25 °C if the concentrations are [Co³+] = 7.60x10-2 M. [Co²+] = 7.80x10-2 M, and [CI-] = 0.475 M, and the pressure of Cl₂ is P₂ = 6.60 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E = Submit HÅ Value Ovide Feedback → Units www. ? Next >
For the reaction 2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl2 (g). E=0.483 V what is the cell potential at 25 °C if the concentrations are [Co³+] = 7.60x10-2 M. [Co²+] = 7.80x10-2 M, and [CI-] = 0.475 M, and the pressure of Cl₂ is P₂ = 6.60 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E = Submit HÅ Value Ovide Feedback → Units www. ? Next >
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![e Nernst equation is one of the most important
ations in electrochemistry. To calculate the cell
cential at non-standard-state conditions, the equation
E = E° 2.303 RT
nF
ere E is the potential in volts, E° is the standard
ential in volts, R is the gas constant, T is the
mperature in kelvins, n is the number of moles of
ctrons transferred, F is the Faraday constant, and Q
he reaction quotient. Using the common reference
mperature, 25 °C or 298 K, the equation has the form
E = E° - (0.0592) log Q
e reaction quotient has the usual form
[products]
[reactants]
F2
-log10 Q
Q =
able of standard reduction potentials gives the voltage
standard conditions, 1.00 M for all solutions and 1.00
m for all gases. The Nernst equation allows for the
culation of the cell potential E at other conditions of
ncentration and pressure.
4,501
80
F3
DEC
7
Q
F4
O
F5
Part A
For the reaction
2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl2 (g). E=0.483 V
what is the cell potential at 25 °C if the concentrations are [Co³+] = 7.60x10-2 M. [Co²+] = 7.80x10-2 M, and [Cl] = 0.475 M,
and the pressure of Cl₂ is P₂ = 6.60 atm ?
Express your answer with the appropriate units.
►View Available Hint(s)
E=
Submit
Value
Provide Feedback
HÅ
C
F6
SO
MacBook Air
- 0
JZA
7
F7
www. ?
Units
DII
F8
F9
X
Review | Constants I Periodic Table
F10
W
zoom
F11
Next >
WA
F12](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fed91748d-3266-4ed4-88a4-c4dd265535d9%2F01860080-1745-4a34-9ca6-b6fd874e60d0%2F5zv17v_processed.jpeg&w=3840&q=75)
Transcribed Image Text:e Nernst equation is one of the most important
ations in electrochemistry. To calculate the cell
cential at non-standard-state conditions, the equation
E = E° 2.303 RT
nF
ere E is the potential in volts, E° is the standard
ential in volts, R is the gas constant, T is the
mperature in kelvins, n is the number of moles of
ctrons transferred, F is the Faraday constant, and Q
he reaction quotient. Using the common reference
mperature, 25 °C or 298 K, the equation has the form
E = E° - (0.0592) log Q
e reaction quotient has the usual form
[products]
[reactants]
F2
-log10 Q
Q =
able of standard reduction potentials gives the voltage
standard conditions, 1.00 M for all solutions and 1.00
m for all gases. The Nernst equation allows for the
culation of the cell potential E at other conditions of
ncentration and pressure.
4,501
80
F3
DEC
7
Q
F4
O
F5
Part A
For the reaction
2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl2 (g). E=0.483 V
what is the cell potential at 25 °C if the concentrations are [Co³+] = 7.60x10-2 M. [Co²+] = 7.80x10-2 M, and [Cl] = 0.475 M,
and the pressure of Cl₂ is P₂ = 6.60 atm ?
Express your answer with the appropriate units.
►View Available Hint(s)
E=
Submit
Value
Provide Feedback
HÅ
C
F6
SO
MacBook Air
- 0
JZA
7
F7
www. ?
Units
DII
F8
F9
X
Review | Constants I Periodic Table
F10
W
zoom
F11
Next >
WA
F12
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