Select the wrong relation `(s)`.

Options

A. `DeltaS=((delE)/(delT))_(P)xxnF`
B. `-DeltaS=((delE)/(delT))_(P)xxnF`
C. `((delE)/(delT))_(P)=((delDeltaS)/(delT))`
D. `((delE)/(delT))_(P)=(DeltaH+nEF)/(T)`

Explanation

To solve the question "Select the wrong relation(s)", we need to analyze each of the given relations based on thermodynamic principles and equations. Let's break down the relations step by step.

### Step 1: Analyze the First Relation
**Relation 1:** \( \Delta S = \frac{\Delta E}{\Delta T} \cdot nF \) at constant pressure.

- This relation suggests that the change in entropy (\( \Delta S \)) is proportional to the change in energy (\( \Delta E \)) divided by the change in temperature (\( \Delta T \)), multiplied by the number of moles (\( n \)) and Faraday's constant (\( F \)).
- This relation is generally correct in the context of electrochemistry where \( \Delta S \) can be related to changes in energy.

**Conclusion:** This relation appears to be correct.

### Step 2: Analyze the Second Relation
**Relation 2:** \( -\Delta S = \frac{\Delta E}{\Delta P} \cdot nF \) at constant pressure.

- This relation suggests that the negative change in entropy is equal to the change in energy divided by the change in pressure, multiplied by \( nF \).
- However, the relationship between entropy and energy changes typically involves temperature, not pressure. This relation does not hold true in standard thermodynamic contexts.

**Conclusion:** This relation is incorrect.

### Step 3: Analyze the Third Relation
**Relation 3:** \( \frac{\Delta E}{\Delta T} \) at constant pressure = \( \frac{\Delta S}{\Delta T} \).

- This relation implies a direct proportionality between the change in energy with respect to temperature and the change in entropy with respect to temperature.
- This is not a standard relation in thermodynamics and does not hold true as stated.

**Conclusion:** This relation is also incorrect.

### Step 4: Analyze the Fourth Relation
**Relation 4:** \( \frac{\Delta E}{\Delta T} \) at constant pressure = \( \frac{\Delta H}{nF} \cdot \frac{1}{T} \).

- This relation suggests that the change in energy with respect to temperature at constant pressure is related to the change in enthalpy (\( \Delta H \)) divided by \( nF \) and temperature.
- This relation can be derived from the Gibbs free energy equation and is consistent with thermodynamic principles.

**Conclusion:** This relation appears to be correct.

### Final Conclusion
The wrong relations are:
- Relation 2: \( -\Delta S = \frac{\Delta E}{\Delta P} \cdot nF \) at constant pressure.
- Relation 3: \( \frac{\Delta E}{\Delta T} \) at constant pressure = \( \frac{\Delta S}{\Delta T} \).