The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N 2 (g)+ 3 H 2 (g) 2 NH 3 (g)or this reaction, ?H° = -92.2 kJ,$\Delta$G° = -33.4 kJ. All things considered, one concludes that

The Answer of The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N 2 (g)+ 3 H 2 (g) 2 NH 3 (g)or this reaction, ?H° = -92.2 kJ,$\Delta$G° = -33.4 kJ. All things considered, one concludes that

The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N 2 (g)+ 3 H 2 (g) 2 NH 3 (g)or this reaction, ?H° = -92.2 kJ,$\Delta$G° = -33.4 kJ. All things considered, one concludes that

The Answer of The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N 2 (g)+ 3 H 2 (g) 2 NH 3 (g)or this reaction, ?H° = -92.2 kJ,$\Delta$G° = -33.4 kJ. All things considered, one concludes that

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The Thermochemical Equation Representing One Process Used for the Synthesis $\Delta$

Question 57

Multiple Choice

The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N₂(g) + 3 H₂(g) $The thermochemical equation representing one process used for the synthesis of ammonia involves the equilibrium shown,N2(g) + 3 H2(g) 2 NH3(g) or this reaction, ?H° = -92.2 kJ, \Delta G° = -33.4 kJ. All things considered, one concludes that A) the coefficients give us the mole ratios but not the volume ratios of the reacting species. B) an increase in pressure favors an increase in the yield of ammonia. C) carrying out the reaction at a higher temperature shifts the position of equilibrium to the right, thus favoring an increase in the yield of ammonia. D) cooling the mixture to remove ammonia from the reaction mixture unfortunately also decreases the overall yield of ammonia. E) the mixture does not need heating, in fact, cooling the mixture assists the rapid establishment of equilibrium.$ 2 NH₃(g) or this reaction, ?H° = -92.2 kJ, $\Delta$ G° = -33.4 kJ. All things considered, one concludes that

A) the coefficients give us the mole ratios but not the volume ratios of the reacting species.
B) an increase in pressure favors an increase in the yield of ammonia.
C) carrying out the reaction at a higher temperature shifts the position of equilibrium to the right, thus favoring an increase in the yield of ammonia.
D) cooling the mixture to remove ammonia from the reaction mixture unfortunately also decreases the overall yield of ammonia.
E) the mixture does not need heating, in fact, cooling the mixture assists the rapid establishment of equilibrium.

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The Thermochemical Equation Representing One Process Used for the Synthesis Δ\DeltaΔ

The Thermochemical Equation Representing One Process Used for the Synthesis $\Delta$