Question

In a reaction$a + b \rightleftharpoons c + d$ will addition of c to the system change the value of K?

Answer 1

"$a\quad +\quad b\quad \rightarrow \quad c\quad +\quad d$

In the above mentioned chemical reaction, the addition of c does not change the value of the equilibrium constant (k). Not only that the change in concentration of the things that present in equilibrium will not disturb the value of equilibrium constant (k). The “temperature” is the “only term” which affect the value of equilibrium."

Answer 2

Answer:

For the reaction,

22−2x

2A(g)

+

22−x

B(g)

⇌

03x

3C(g)

+

0x

D

(g)

2 moles each of A and B were taken into a flask. The consumption of A is twice of that of B.

Hence, [A]

eqm

<[B]

eqm

Also from the reaction stoichiometry,

−

2

1

dt

d

[A]=−

dt

d

[B]

or

−

dt

d

[A]=−2

dt

d

[B]

The rate of consumption of A is twice the rate of consumption of B.

So the equilibrium concentration of A will be less than the equilibrium concentration of B.

Option B is correct.