5) Using the Nernst Expression, Eobs background reading when T = 20.4°C, and the concentrations are . .. E° -RT/nF InQ , calculate Ehe for the reaction n the 'obs %3D a) [Cu²*]= 0.10M, [Zn*] = 0.25M %3D b) [Cu*] = 0.37M , [Zn"] = 0.20M %3D c) [Cu] = 0.10M , [Zn²"] = 0.01M
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
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![Transcription and Explanation for Educational Website:
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**Exercise: Calculating Electrode Potential Using the Nernst Equation**
**Problem Statement:**
Using the Nernst Expression, \(E_{\text{obs}} = E^0 - \frac{RT}{nF} \ln Q\), calculate \(E_{\text{obs}}\) for the reaction in the background when the temperature \(T = 20.4^\circ C\) and the concentrations are as follows:
1. **Case a:**
- \([\text{Cu}^{2+}] = 0.10\, M\)
- \([\text{Zn}^{2+}] = 0.25\, M\)
2. **Case b:**
- \([\text{Cu}^{2+}] = 0.37\, M\)
- \([\text{Zn}^{2+}] = 0.20\, M\)
3. **Case c:**
- \([\text{Cu}^{2+}] = 0.10\, M\)
- \([\text{Zn}^{2+}] = 0.01\, M\)
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**Note:**
The Nernst equation is used to calculate the electric potential (voltage) of an electrochemical cell under non-standard conditions. The formula requires the standard electrode potential \(E^0\), the temperature \(T\), the universal gas constant \(R\), the Faraday constant \(F\), the number of moles of electrons transferred in the reaction \(n\), and the reaction quotient \(Q\), which is calculated from the concentration of the reactants and products involved in the cell reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F88f794be-122d-44d8-bdbd-e59efaff39a0%2F0c72ff76-0840-4a22-ab40-1590d03a48ee%2Fri4uku5.jpeg&w=3840&q=75)
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