Question

For the given reaction, which of the following is true?

N_2 (g) + 3H_2 (g) rightarrow 2NH_3 (g)

a) The reaction is exothermic.
b) The reaction is endothermic.
c) The equilibrium constant ((K_c)) is temperature-dependent.
d) The reaction produces a higher concentration of reactants at equilibrium.

Answer 1

The reaction N₂(g) + 3H₂(g) ⇒ 2NH₃(g) is exothermic and the equilibrium constant Kc is temperature-dependent, but the reaction does not produce a higher concentration of reactants at equilibrium.

Step-by-step explanation:

The reaction N₂ (g) + 3H₂ (g) ⇒ 2NH₃ (g) is exothermic, as it releases heat. The option 'a)' incorrectly stating the reaction is exothermic is not true for this specific chemical equation provided, which is actually exothermic in nature. Furthermore, the equilibrium constant (Kc) is indeed dependent on temperature, making option 'c)' true. Lastly, at equilibrium, this reaction does not produce a higher concentration of reactants but rather products, making option 'd)' incorrect.

Regarding the equilibrium constant, it's noteworthy that the value of Kc doesn't change with changes in concentrations of reactants or products, but it does change with temperature. Therefore, the reaction does not produce a higher concentration of reactants at equilibrium as stated in option 'd)'; instead, it results in a higher concentration of ammonia, NH₃.