Question

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Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK

Answer 1

Q1. Fe₂O₃ (s) + 3 H₂ (g) $\rightarrow$ 2 Fe (s) + 3 H₂O (g)

$\Delta$S^o_system = 337.7 J/K

Q2. 2 CO (g) + O₂ (g) $\rightarrow$ 2 CO₂ (g)

$\Delta$S^o_system = -133.3 J/K

Q3. 2 NH₃ (g) + 3 N₂O (g) $\rightarrow$ 4 N₂ (g) + 3 H₂O (g)

The standard free energy change for the reaction of 2.45 moles of NH₃ (g) at 316 K, 1 atm would be -1188.9 kJ.

This reaction is product favored under standard conditions at 316 K.

Q4. H₂ (g) + C₂H₄ (g) $\rightarrow$ C₂H₆ (g)

This reaction is product favored under standard conditions at 298 K.

The standard enthalpy change for the reaction of 2.45 moles of NH₃ (g) at 316 K, 1 atm would be -300 kJ