Question

Consider the following reaction at room temperature: 2X(g) ⇌ 2Y(g) + Z(g) Kc = 2.0 x 10-5

                  If you put 0.28 mol of X, 0.050 mol of Y, and 0.080 mol of Z into a 5 L container what happens to the reaction?

	a.	the reaction will proceed forward
	b.	the reaction will proceed backwards
	c.	the reaction will go to completion
	d.	the reaction will be at equilibrium

Answer 1

Answer: (a) reaction will proceed forward ,is correct option

explanation:

the given reaction is ;

2X(g) ⇌ 2Y(g) + Z(g)

Kc = 2.0 x 10-5 (given)

When we put the given moles of X, Y, and Z , we first calculate the concentration of X,Y, Z

[X] = 0.28 mole / 5 L = 0.056 M

[Y] = 0.050 mole / 5L = 0.01 M

[Z] = 0.080 mole /5L = 0.016 M

Expression for Q, will be :

Q = [Y]^2*[Z] / [X]^2

=( 0.01)^2 * 0.016 / (0.056)^2

= 0.00051 = 5.1*10^-4

Since , Kc > Q

Therefore, the reaction will proceed forward.

And , (a) option is correct

please upvote