For the reaction H2(g) + 1/2 O2(g) - H2O(l) at 298 K, Delta_r G deg = -237.1 kJ mol^-1 and Delta_r H deg = -285.8 kJ mo

Question

For the reaction H2(g) + 1/2 O2(g) -> H2O(l) at 298 K, Delta_r G deg = -237.1 kJ mol^-1 and Delta_r H deg = -285.8 kJ mol^-1. A hydrogen-oxygen fuel cell is based on this reaction. Take F = 96500 C mol^-1. Which statements are correct?

Accepted Answer

The standard EMF of the cell is about 1.23 V

Accepted Answer

The maximum thermodynamic efficiency of the cell is about 83%

Accepted Answer

Delta_r S deg for the reaction is about -163 J K^-1 mol^-1

Answer

If the cell operates at 0.70 V, the heat released to the surroundings per mole of H2 is about 102 kJ

For the reaction $H X_{2} (g) + \frac{1}{2} O X_{2} (g) H X_{2} O (l)$ at 298 K, $Δ_{r} G^{\circ} = - 237.1 kJ mo l^{- 1}$ and $Δ_{r} H^{\circ} = - 285.8 kJ mo l^{- 1}$ . A hydrogen-oxygen fuel cell is based on this reaction. Take $F = 96500 C mo l^{- 1}$ . Which statements are correct?

Answer: A, C, D

More questions on Fuel cells

For the reaction HX2​(g)+21​OX2​(g)​HX2​O(l) at 298 K, Δr​G∘=−237.1 kJmol−1 and Δr​H∘=−285.8 kJmol−1. A hydrogen-oxygen fuel cell is based on this reaction. Take F=96500 Cmol−1. Which statements are correct?

Answer: A, C, D

More questions on Fuel cells

For the reaction $H X_{2} (g) + \frac{1}{2} O X_{2} (g) H X_{2} O (l)$ at 298 K, $Δ_{r} G^{\circ} = - 237.1 kJ mo l^{- 1}$ and $Δ_{r} H^{\circ} = - 285.8 kJ mo l^{- 1}$ . A hydrogen-oxygen fuel cell is based on this reaction. Take $F = 96500 C mo l^{- 1}$ . Which statements are correct?