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A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0?
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A cellreaction would be spontaneous if the cell potential and delta rG...
E = - ∆G/nF
as the Cell potential is positive , the change in Gibbs free energy become negative , The reaction becomes spontaneous.
as the Cell potential is positive , the change in Gibbs free energy become negative , The reaction becomes spontaneous.
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A cellreaction would be spontaneous if the cell potential and delta rG...
Spontaneity of a Cell Reaction
The spontaneity of a cell reaction can be determined by comparing the cell potential (Ecell) and the change in Gibbs free energy (ΔrG) of the reaction. The sign of Ecell and ΔrG provides information about the spontaneity of the reaction.
1. Ecell and ΔrG both negative (-ve -ve)
- If the cell potential (Ecell) is negative and the change in Gibbs free energy (ΔrG) is also negative, then the cell reaction is spontaneous.
- A negative value for Ecell indicates that the reaction proceeds in the forward direction.
- A negative value for ΔrG indicates that the reaction is exergonic, meaning it releases energy.
- Therefore, when both Ecell and ΔrG are negative, the cell reaction is spontaneous.
2. Ecell and ΔrG both positive (+ve +ve)
- If the cell potential (Ecell) is positive and the change in Gibbs free energy (ΔrG) is also positive, then the cell reaction is non-spontaneous.
- A positive value for Ecell indicates that the reaction proceeds in the reverse direction.
- A positive value for ΔrG indicates that the reaction is endergonic, meaning it requires energy input.
- Therefore, when both Ecell and ΔrG are positive, the cell reaction is non-spontaneous.
3. Ecell is zero and ΔrG is zero (0 0)
- If the cell potential (Ecell) is zero and the change in Gibbs free energy (ΔrG) is also zero, then the spontaneity of the reaction cannot be determined solely by these values.
- A cell potential of zero indicates that the reaction is at equilibrium.
- A change in Gibbs free energy of zero indicates that the reaction neither releases nor requires energy.
- The spontaneity of the reaction in this case depends on other factors such as the concentrations of reactants and products.
Conclusion
In summary, a cell reaction is spontaneous when both the cell potential (Ecell) and the change in Gibbs free energy (ΔrG) are negative. If both values are positive, the reaction is non-spontaneous. However, if Ecell is zero and ΔrG is zero, the spontaneity of the reaction cannot be determined solely based on these values.
The spontaneity of a cell reaction can be determined by comparing the cell potential (Ecell) and the change in Gibbs free energy (ΔrG) of the reaction. The sign of Ecell and ΔrG provides information about the spontaneity of the reaction.
1. Ecell and ΔrG both negative (-ve -ve)
- If the cell potential (Ecell) is negative and the change in Gibbs free energy (ΔrG) is also negative, then the cell reaction is spontaneous.
- A negative value for Ecell indicates that the reaction proceeds in the forward direction.
- A negative value for ΔrG indicates that the reaction is exergonic, meaning it releases energy.
- Therefore, when both Ecell and ΔrG are negative, the cell reaction is spontaneous.
2. Ecell and ΔrG both positive (+ve +ve)
- If the cell potential (Ecell) is positive and the change in Gibbs free energy (ΔrG) is also positive, then the cell reaction is non-spontaneous.
- A positive value for Ecell indicates that the reaction proceeds in the reverse direction.
- A positive value for ΔrG indicates that the reaction is endergonic, meaning it requires energy input.
- Therefore, when both Ecell and ΔrG are positive, the cell reaction is non-spontaneous.
3. Ecell is zero and ΔrG is zero (0 0)
- If the cell potential (Ecell) is zero and the change in Gibbs free energy (ΔrG) is also zero, then the spontaneity of the reaction cannot be determined solely by these values.
- A cell potential of zero indicates that the reaction is at equilibrium.
- A change in Gibbs free energy of zero indicates that the reaction neither releases nor requires energy.
- The spontaneity of the reaction in this case depends on other factors such as the concentrations of reactants and products.
Conclusion
In summary, a cell reaction is spontaneous when both the cell potential (Ecell) and the change in Gibbs free energy (ΔrG) are negative. If both values are positive, the reaction is non-spontaneous. However, if Ecell is zero and ΔrG is zero, the spontaneity of the reaction cannot be determined solely based on these values.
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A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0?
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A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0?.
A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A cellreaction would be spontaneous if the cell potential and delta rG are respectively? 1. ve -ve 2.-ve -ve 3.0 0 ve 0?.
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