Question

When 4.00 mol of each X(g) and Y(g) are placed in a 1.00 L vessel and allowed to react at constant temperature according to the equation below, 6.00 mol of Z(g) is produced. What is the value of the equilibrium constant, Kc?

X(g) + Y(g) ---> 2 Z(g)


8
16
36
6

Answer 1

Answer: The value of equilibrium constant for the above equation is 36

Explanation:

We are given:

Initial moles of X = 4.00 moles

Initial moles of Y = 4.00 moles

Equilibrium moles of Z = 6.00 moles

Volume of vessel = 1.00 L

Initial concentration of X = $\frac{4}{1}=4$

Initial concentration of Y = $\frac{4}{1}=4$

Equilibrium concentration of Z = $\frac{6}{1}=6$

The given chemical equation follows:

                  $X(g)+Y(g)\rightarrow 2Z(g)$

Initial:         4         4

At eqllm:     4-x      4-x        2x

Calculating for 'x', we get:

$\Rightarrow 2x=6\\\\\Rightarrow x=3$

The expression of $K_c$ for above equation follows:

$K_c=\frac{[Z]^2}{[X]\times [Y]}$

Putting values in above equation, we get:

$K_c=\frac{6^2}{1\times 1}\\\\K_c=36$

Hence, the value of equilibrium constant for the above equation is 36