Consider the following reactionN2(g) + 3H2(g) ⇌ 2NH3(g) ΔH°rxn = –92 kJWhich one of the following statements about this reaction is correct? A. A plot of ln K vs. (1/T) will be a straight line with a negative slope. B. Compression of the system will shift the equilibrium to the left. C. ½ ΔH°rxn is equal to the standard enthalpy of formation of NH3(g). D. An increase in temperature will shift the equilibrium to the right. E. Addition of N2(g) at constant temperature will increase the equilibrium constant.

The given reaction is saber process of ammonia formation. This reaction is an exothermic reaction.

Answered: Consider the following reaction N2(g) +…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...

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Question

Consider the following reaction

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) ΔH°_rxn = –92 kJ

Which one of the following statements about this reaction is correct?

A.
A plot of ln K vs. (1/T) will be a straight line with a negative slope.
B.
Compression of the system will shift the equilibrium to the left.
C.
½ ΔH°_rxn is equal to the standard enthalpy of formation of NH₃(g).
D.
An increase in temperature will shift the equilibrium to the right.
E.
Addition of N₂(g) at constant temperature will increase the equilibrium constant.

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