Electrochemical Cells

Step 1: Write the combustion reaction of butane: Step 2: Calculate the standard Gibbs free energy change for the reaction using standard Gibbs energies of formation: Note: of is zero (elemental form). Step 3: Calculate the cell potential using the relation: Where, = number of electrons transferred, = Faraday constant, = cell potential in volts. Step 4: Find , the total electrons involved in the reaction. The combustion of butane involves oxidation of carbon from 0 in butane to +4 in . - Butane has 4 carbon atoms; each carbon is oxidized by losing 4 electrons (from 0 to +4 oxidation state). - Total electrons transferred, Step 5: Calculate : Step 6: Given the cell potential is volts, we rewrite the above as: Multiply both sides by and divide by : Step 7: Based on the problem context and the options provided, the closest match for is 3.87.

Step 1: Write the combustion reaction of butane: Step 2: Calculate the standard Gibbs free energy change for the reaction using standard Gibbs energies of formation: Note: of is zero (elemental form). Step 3: Calculate the cell potential using the relation: Where, = number of electrons transferred, = Faraday constant, = cell potential in volts. Step 4: Find , the total electrons involved in the reaction. The combustion of butane involves oxidation of carbon from 0 in butane to +4 in . - Butane has 4 carbon atoms; each carbon is oxidized by losing 4 electrons (from 0 to +4 oxidation state). - Total electrons transferred, Step 5: Calculate : Step 6: Given the cell potential is volts, we rewrite the above as: Multiply both sides by and divide by : Step 7: Based on the problem context and the options provided, the closest match for is 3.87.