Calculate E^∘ at 25^∘ C for fuel cells utilizing the reactions (a) C2 H6(g)+3 (1)/(2) O2(g)=2

step 1 Let's calculate delta g -not for each of the following reactions for a reaction is n2 gas plus o

Calculate E^∘ at 25^∘ C for fuel cells utilizing the...

Calculate $E^{\circ}$ at $25^{\circ} \mathrm{C}$ for fuel cells utilizing the reactions $(a) \quad \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g})+3 \frac{1}{2} \mathrm{O}_{2}(\mathrm{g})=2 \mathrm{CO}_{2}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ $(b) \quad \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g})=2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ Catalysts have not yet been developed to make these fuel cells possible.

Calculate $E^{\circ}$ at $25^{\circ} \mathrm{C}$ for fuel cells utilizing the reactions
$(a) \quad \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g})+3 \frac{1}{2} \mathrm{O}_{2}(\mathrm{g})=2 \mathrm{CO}_{2}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$
$(b) \quad \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g})=2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ Catalysts have not yet been developed to make these fuel cells possible.

Key Concepts

Standard Electrode Potential

The standard electrode potential (E°) is a measure of the intrinsic tendency of a chemical species to be reduced, under standard conditions (25°C, 1 atm, and 1 M concentrations). In the context of fuel cells, the overall cell potential is calculated as the difference between the cathode and anode potentials.

Relationship Between Gibbs Free Energy and Cell Potential

The relationship between the standard Gibbs free energy change (?G°) and the cell potential (E°) is given by the equation ?G° = -nFE°. This formula connects the thermodynamic favorability of a reaction to the electrical work that can be obtained, with n representing the number of electrons transferred in the redox process and F the Faraday constant.

Fuel Cells

Fuel cells are devices that convert the chemical energy stored in fuels directly into electrical energy through redox reactions. They operate by accepting electrons at the anode and passing them through an external circuit to the cathode where they participate in reduction reactions, thus creating an electrical current.

Reaction Stoichiometry

Reaction stoichiometry involves the balancing of chemical equations to determine the number of electrons exchanged during a redox reaction. Understanding the stoichiometry is crucial for calculating the number of electrons (n) involved, which is a key factor when using the ?G° = -nFE° relationship to find the cell potential.

Transcript

Please give Ace some feedback