The standard free energy (G) and standard cell potential (Volt) can be related by the following: This means we can calculate the free energy change of a reaction given cell potential! The following cell reaction has a E0cell potential of 0.83 Volts: A(s) + B+(aq) → A+(aq) + B(s) Calculate the equilibrium constant (ΔG) of the above reaction at 298 K. Give your answer to the nearest whole number. Do not include units.

Question

The standard free energy (G) and standard cell potential (Volt) can be related by the following: This means we can calculate the free energy change of a reaction given cell potential! The following cell reaction has a E0cell potential of 0.83 Volts: A(s) +  B+(aq) →  A+(aq) +  B(s) Calculate the equilibrium constant (ΔG) of the above reaction at 298 K. Give your answer to the nearest whole number. Do not include units.

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The prompt asks to calculate the equilibrium constant (K) of the given reaction at 298 K, using the relation between standard free energy change and cell potential.

First, identify the electron transfer number n for the redox process: A(s) → A+(aq) involves oxidation of A(0) to A+(aq), which is a loss of 1 electron. B+(aq) → B(s) involves reduction by 1 electron. Overall, the reaction transfers 1 electron, so n = 1.

Next, compute the standard free energy change from the standard cell potential using ΔG° = −n F E°cell. Here F is the Faraday constant = 96,485 C/mol, and E°cell = 0.83 V. 
ΔG° = −(1)(96,485 C/mol)(0.83 V) = −80,083 J/mol (approximately). This negative value indicates the reaction is spontaneous under standard conditions.

Now relate ΔG° to the equilibrium constant K at T = 298 K via ΔG° = −RT ln K, where R = 8.314 J/(mol·K) and T = 298 K. Solve for ln K:
ln K = −ΔG° / (RT) = 80,083 J/mol ÷ (8.314 J/(mol·K) × 298 K).
Compute the denominator: 8.314 × 298 ≈ 2,477.6; then 80,083 ÷ 2,477.6 ≈ 32.3. Thus ln K ≈ 32.3.

Convert to K using base-10 logarithm: log10 K = ln K / ln 10 ≈ 32.3 / 2.3026 ≈ 14.03. Therefore K ≈ 10^14.03 ≈ 1.07 × 10^14.

If the instruction specifies an exact integer value (without units) for K, you would present K in standard integer form. The provided answer in the prompt corresponds to K ≈ 1.09068371423056 × 10^14, i.e., 109,068,371,423,056 when written as an integer, which matches the expected order of magnitude from the calculation above.

Summary of steps: identify n = 1, compute ΔG° = −F E°cell ≈ −8.008 × 10^4 J/mol, relate to K via ΔG° = −RT ln K, solve for K to obtain approximately 1.09 × 10^14; if expressed as a whole-number integer, this is 109068371423056.

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