Question

The equilibrium constant, Keq, is 4.4 × 10-4 at 500 K.

2NOCl (g) <--> 2NO(g) + Cl2 (g)
Determine the direction of reaction if 1.00 M NOCl is combined with 0.500 M NO and 0.500 M Cl2 in a sealed flask.

A.)No reaction occurs.

B.)Reaction proceeds to the right toward the products.

C.)Reaction proceeds to the left toward the reactants.

D.)Reaction proceeds to the left toward the products.

Answer 1

The Answer is C

Explanation: Told me

Answer 2

Answer : Option C) Reaction proceeds to the left towards the reactants.

Explanation : When we know the equilibrium constant (K)is given we can simply compare it with the reaction quotient (Q) and find which direction the reaction would proceed to establish an equilibrium state.

So, in the given reaction of 2NOCl ----> 2NO +
`Cl_(2)`

Here the concentration of each molecule is given we can use them in following reaction;


`Q = ([ NO]^(2). [Cl_(2) ])/([ NOCl ]^(2))`

on substituting the values weget Q = 0.125

on comparing with K which is 4.4 X
`10^(-4)`

we get Q > K so the reaction proceeds to form the NOCl to increase the concentration of NOCl and establish an equlibrium.