For N2(g) + 3H2(g) 2NH3(g), Delta H = -92 kJ. On raising the temperature of the equilibrium mixture,

the equilibrium shifts backward and K decreases

the equilibrium is unaffected because Delta n neq 0

the equilibrium shifts backward and K decreases

the equilibrium shifts backward but K is unchanged

the equilibrium shifts forward and K increases

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NEET levelSingle correct optionDifficulty 1 of 3ce171

For $N X_{2} (g) + 3 H X_{2} (g) 2 NH X_{3} (g)$ , $Δ H = - 92 kJ$ . On raising the temperature of the equilibrium mixture,

Athe equilibrium is unaffected because $Δ n \neq = 0$
Bthe equilibrium shifts backward and $K$ decreases
Cthe equilibrium shifts backward but $K$ is unchanged
Dthe equilibrium shifts forward and $K$ increases

Answer: B

Heat is absorbed by the endothermic (reverse) reaction, so the equilibrium shifts backward. The equilibrium constant of an exothermic reaction decreases with temperature.

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For NX2​(g)+3HX2​(g)​2NHX3​(g), ΔH=−92 kJ. On raising the temperature of the equilibrium mixture,

Answer: B

More questions on Le Chatelier's principle: effect of concentration, pressure, temperature, inert gas

For $N X_{2} (g) + 3 H X_{2} (g) 2 NH X_{3} (g)$ , $Δ H = - 92 kJ$ . On raising the temperature of the equilibrium mixture,