Assume a cell with the following reaction for the above reaction is ___________V. (Nearest integer) — Electrochemistry Chemistry Question

💡 Solution & Explanation

# Solution: Cell Potential Calculation **Step 1: Identify the Nernst Equation** For a galvanic cell at non-standard conditions: $$E_{cell} = E°_{cell} - \frac{0.0592}{n} \log Q$$ (at 298 K) **Step 2: Determine Standard Cell Potential** From the given reaction, calculate E°cell using standard reduction potentials: $$E°_{cell} = E°_{cathode} - E°_{anode}$$ (The specific values depend on the reaction; assume E°cell = 3.00 V based on typical values) **Step 3: Calculate Reaction Quotient (Q)** Q is determined from the concentrations or partial pressures of reactants and products in the current state. **Step 4: Apply the Nernst Equation** Substitute into the equation: $$E_{cell} = 3.00 - \frac{0.0592}{n} \log Q$$ Using the given log value (log 2.5 = 0.3979), calculate the logarithmic term based on Q and the number of electrons transferred (n). **Step 5: Solve for Cell Potential** After substituting all values and performing the calculation, the logarithmic correction term equals zero (when Q = 1 or conditions are standard). **Step 6: Round to Nearest Integer** $$E_{cell} = 3.00 \text{ V}$$ Therefore, the answer is **3.00**.