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For which reaction, carried out at standard conditions, wouldboth the enthalpy and entropy changes drive the reaction in thesame direction? Please EXPLAIN.

A. 2H2(g) + O2(g) --->2H2O(l) ΔH = -571.1 kJ

B. 2Na(s) + Cl2(g)---->2NaCl(s) ΔH = -822.0kJ

C. N2(g) + 2O2(g) ---->2NO2(g) ΔH= +67.7 kJ

D. 2NH3(g) ----> N2(g) +3H2(g) ΔH= +92.4 kJ

Answer :

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Answer:

2NH3(g) ----> N2(g) +3H2(g) ΔH= +92.4 kJ

Explanation:

Entropy increases with increase in the number of particles from left to right in a reaction. Hence, the reaction; 2NH3(g) ----> N2(g) +3H2(g) ΔH= +92.4 kJ is favoured by increase in entropy.

Similarly, the enthalpy change for the reaction is only +92.4 KJ. Hence for this reaction, both enthalpy and entropy changes drive the reaction in the same direction.

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