A reversible reaction is studied graphically as shown in the given figure.
$N_{2} O_{4} ⇌ 2 N O_{2}, K_{c} = 4$
Select the correct statements out of I, II and III.
I. Reaction quotient has maximum value at point A.
II. Reaction proceeds left to right at a point when $[N_{2} O_{4}] = [N O_{2}] = 0.1$ M.
III. $K_{c} = Q$ when point D or F is reached.

I, II

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II, III

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I, III

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I, II, III

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Solution

The correct option is A II, III
The given reaction is :-
$N_{2} O_{4} ⇌ 2 {N O}_{2}, K_{C} = 4$

Now, we have, $Q_{C} = \frac{{[{N O}_{2}]}^{2}}{[N_{2} O_{4}]}$

$(1)$ Now, at $A$ , $[{N O}_{2}]$ is minimum & $[N_{2} O_{4}]$ is maximum, so, $Q_{C}$ will be minimum at point $A$ .

$(2)$ when $[N_{2} O_{4}] = [{N O}_{2}] = 0.1 M$

$Q_{C} = \frac{{(0.1)}^{2}}{0.1} = 0.1 & K_{C} = 4$

$\Rightarrow Q_{C} < K_{C} \Rightarrow$ Reaction will proceed towards product i.e. from left to right.

$(3)$ $K_{C} = Q$ when equilibrium is reached.

$\Rightarrow \frac{{[{N O}_{2}]}^{2}}{[N_{2} O_{4}]} = 4$

$\Rightarrow {[{N O}_{2}]}^{2} = 4 [N_{2} O_{4}]$

so, it is the condition at point $D$ or $F$ .

Suggest Corrections

Similar questions

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{C} = 4

This reversible reaction is studied graphically as shown in figure. Select correct statements out of I, II and III
(I) Reaction quotient has maximum value at point A.
(II) Reaction proceeds from left to right at a point when,

[N_{2} O_{4}] = [N O_{2}] = 0.1 M

.
(III)

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. This reversible reaction is studied graphically as shown in figure. Select the correct statements out of I, II and III.
I: Reaction quotient has maximum value at point

A

II: Reaction proceeds left to right at a point when

[N_{2} O_{4}] = [N O_{2}] = 0.1 M

III:

K_{c} = Q

when a point

D

F

is reached.

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{C} = 4

[N_{2} O_{4}] = [N O_{2}] = 0.1 M

.
(III)

K_{c} = Q

, when point D or F is reached

The reaction N $_{2}$ O $_{4}$ (g) $⇌$ 2NO $_{2}$ (g) is
carried out at 298 K and 20 bar. Five moles of each of N $_{2}$ O $_{4}$ and
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(N $_{2}$ O $_{4}$ ) = 100 kJ mol $^{- 1}$ and $Δ$ $_{f}$ G $^{\circ}$
(NO $_{2}$ ) = 50 kJ mol $^{- 1}$ . The reaction proceeds at an initial pressure
of 20 bar. Determine the direction in which the reaction proceeds to achieve
equilibrium. Also determine the amounts of N $_{2}$ O $_{4}$ and NO $_{2}$ when the reaction attains equilibrium.