Problem: For which reaction, carried out at standard conditions, would both the enthalpy and entropy changes drive the reaction in the same direction? a) 2 H2 (g) + O2 (g) → 2 H2O (l)         ΔH = - 571.1 kJ b) 2 Na (s) + Cl2 (g) → 2 NaCl (s)      ΔH = - 822.0 kJ c) N2 (g) + 2 O2 (g) → 2 NO2 (g)        ΔH = + 67.7 kJ d) 2 NH3 (g) → N2 (g) + 3 H2 (g)        ΔH = + 92.4 kJ

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For which reaction, carried out at standard conditions, would both the enthalpy and entropy changes drive the reaction in the same direction?

a) 2 H(g) + O(g) → 2 H2O (l)         ΔH = - 571.1 kJ

b) 2 Na (s) + Cl(g) → 2 NaCl (s)      ΔH = - 822.0 kJ

c) N(g) + 2 O(g) → 2 NO(g)        ΔH = + 67.7 kJ

d) 2 NH(g) → N(g) + 3 H(g)        ΔH = + 92.4 kJ

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