Question

Ammonia can be produced via the chemicalreaction

\rm N_2 (g) + 3 H_2 (g) \rightleftharpoons 2 NH_3 (g)
During the production process, the production engineer determinesthe reaction quotient to be Q_2 = 3.56Ã10â4. IfK_2 = 6.02Ã10â2, what can besaid about the reaction?
1)The reaction has reached equilibrium.
2)The reaction is not at equilibrium and willproceed to the left.
3)The reaction is not at equilibrium and willproceed to the right.
4)The reaction is not at equilibrium, but it isnot possible to determine whether the reaction needs to proceedright or left to reach equilibrium.

Answer 1

3)The reaction is not at equilibrium and willproceed to the right.

Step-by-step explanation:

The reaction quotient of an equilibrium reaction measures relative amounts of the products and the reactants present during the course of the reaction at particular point in the time.

It is the ratio of the concentration of the products and the reactants each raised to their stoichiometric coefficients. The concentration of the liquid and the gaseous species does not change and thus is not written in the expression.

Q < Kc , reaction will proceed in forward direction.

Q > Kc , reaction will proceed in backward direction.

Q = Kc , reaction at equilibrium.

Given that:

Q =
`3.56* 10^(-4)`

K =
`6.02* 10^(-2)`

Since, Q < K , reaction is not at equilibrium and will proceed to right, in forward direction.