Question

If the reaction is carried out in a 22.4 L container, which initial amounts of X and Y will result in the formation of solid XY? If the reaction is carried out in a 22.4 container, which initial amounts of and will result in the formation of solid ? 2.0 mol X; 2.0 molY 6 mol X; 0.6 molY 1 mol X; 1 molY none of the above

Answer 1

This is an incomplete question, here is the complete question.

The solid XY decomposes into gaseous X and Y:  

$XY(s)\rightleftharpoons X(g)+Y(g)$    Kp = 4.1 (at 0°C)

If the reaction is carried out in a 22.4 L container, which initial amounts of X and Y will result in the formation of solid XY?

a) 2.0 mol X; 2.0 mol Y

b) 6 mol X; 0.6 mol Y

c) 1 mol X; 1 mol Y

d) None of the above

Answer : The correct option is, (D) None of the above

Explanation :

Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

$XY(s)\rightleftharpoons X(g)+Y(g)$

The expression for reaction quotient will be :

Q = [X] [Y]

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

The given equilibrium constant value is, $K_p=4.1$

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

If the initial amount of X and Y to form XY then the product of their product must be greater than Kp.

Now we have to calculate the product of partial pressure.

PV = nRT

$P=\frac{nRT}{V}$

Moles of X      Moles of Y      Pressure of X     Pressure of Y       Q

   2.0                    2.0                  2.00                   2.00                4.00

    6                       0.6                 6.00                    0.6                  3.6

    1                         1                     1.00                    1.00                 1.00

There are 3 conditions:

When $Q>K_c$ that means product > reactant. So, the reaction is reactant favored.

When $Q<K_c$ that means reactant > product. So, the reaction is product favored.

When $Q=K_c$ that means product = reactant. So, the reaction is in equilibrium.

From the above we conclude that, in all the three options $Q<K_c$ that means product < reactant. So, the reaction is product favored that means reaction must shift to the product (right) to be in equilibrium. That means the reaction will not move to the left to form XY.

Hence, the correct option is, (D)