6. Chemical Quantities & Aqueous Reactions
Redox Reactions
6. Chemical Quantities & Aqueous Reactions Redox Reactions
49PRACTICE PROBLEM
Molten carbonate fuel cells (MCFC) are newly developed fuel cells that commonly use molten lithium and potassium carbonates as electrolytes. The half-reactions in the cell are shown below:
Anode: H2(g) + CO32–(l) → H2O(l) + CO2(g) + 2 e–
Cathode: 1/2 O2(g) + CO2(g) + 2 e– → CO32–(l)
Using the thermodynamic values below, determine the cell potential (E°) and the equilibrium constant (K) for the overall reaction at 25°C. Identify whether the values of E° and K will increase, decrease or remain unchanged as the temperature decreases.
Molten carbonate fuel cells (MCFC) are newly developed fuel cells that commonly use molten lithium and potassium carbonates as electrolytes. The half-reactions in the cell are shown below:
Anode: H2(g) + CO32–(l) → H2O(l) + CO2(g) + 2 e–
Cathode: 1/2 O2(g) + CO2(g) + 2 e– → CO32–(l)
Using the thermodynamic values below, determine the cell potential (E°) and the equilibrium constant (K) for the overall reaction at 25°C. Identify whether the values of E° and K will increase, decrease or remain unchanged as the temperature decreases.