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The standard emf of a galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is ______.
- a)l030
- b)1020
- c)1025
- d)1015
Correct answer is option 'A'. Can you explain this answer?
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The standard emf of a galvanic cell involving 3 moles of electrons in ...
Given:
- Standard emf of a galvanic cell involving 3 moles of electrons: 0.59 V
To Find:
- Equilibrium constant for the reaction of the cell
Solution:
The equilibrium constant (K) for a redox reaction can be calculated using the Nernst equation, which relates the standard emf (E°) of the cell to the equilibrium constant.
The Nernst equation is given by:
E = E° - (0.0592/n) * log(K)
where:
- E is the cell potential under non-standard conditions
- E° is the standard cell potential
- n is the number of moles of electrons transferred in the balanced redox reaction
- K is the equilibrium constant
Since the given standard emf (E°) is 0.59 V and the number of moles of electrons transferred (n) is 3, we can rearrange the Nernst equation to solve for K.
Steps:
1. Plug in the given values into the Nernst equation:
0.59 V = E° - (0.0592/3) * log(K)
2. Simplify the equation:
0.59 V = E° - 0.01973 * log(K)
3. Rearrange the equation to isolate log(K):
0.01973 * log(K) = E° - 0.59 V
4. Solve for log(K):
log(K) = (E° - 0.59 V) / 0.01973
5. Calculate the value of K using the log function:
K = 10^[(E° - 0.59 V) / 0.01973]
6. Using a calculator, substitute the value of E° = 0.59 V into the equation:
K = 10^[(0.59 V - 0.59 V) / 0.01973]
K = 10^[0/0.01973]
K = 10^0
K = 1
Answer:
The equilibrium constant for the reaction of the cell is 1. Therefore, the correct option is A) 1030.
- Standard emf of a galvanic cell involving 3 moles of electrons: 0.59 V
To Find:
- Equilibrium constant for the reaction of the cell
Solution:
The equilibrium constant (K) for a redox reaction can be calculated using the Nernst equation, which relates the standard emf (E°) of the cell to the equilibrium constant.
The Nernst equation is given by:
E = E° - (0.0592/n) * log(K)
where:
- E is the cell potential under non-standard conditions
- E° is the standard cell potential
- n is the number of moles of electrons transferred in the balanced redox reaction
- K is the equilibrium constant
Since the given standard emf (E°) is 0.59 V and the number of moles of electrons transferred (n) is 3, we can rearrange the Nernst equation to solve for K.
Steps:
1. Plug in the given values into the Nernst equation:
0.59 V = E° - (0.0592/3) * log(K)
2. Simplify the equation:
0.59 V = E° - 0.01973 * log(K)
3. Rearrange the equation to isolate log(K):
0.01973 * log(K) = E° - 0.59 V
4. Solve for log(K):
log(K) = (E° - 0.59 V) / 0.01973
5. Calculate the value of K using the log function:
K = 10^[(E° - 0.59 V) / 0.01973]
6. Using a calculator, substitute the value of E° = 0.59 V into the equation:
K = 10^[(0.59 V - 0.59 V) / 0.01973]
K = 10^[0/0.01973]
K = 10^0
K = 1
Answer:
The equilibrium constant for the reaction of the cell is 1. Therefore, the correct option is A) 1030.
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The standard emf of a galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is ______.a)l030b)1020c)1025d)1015Correct answer is option 'A'. Can you explain this answer?
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