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Standard XI

Chemistry

Reaction Quotient

N2O4g ⇌ 2NO2g...

Question

$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{C} = 4$
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) $K_{c} = Q$ , 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 B II, III
$N_{2} O_{4} ⇌ 2 N O_{2}; K_{C} = 4$
(I) At point - A,
$Q = \frac{[Product]}{[Reactant]} = 0$
So, Q have minimum value at point A.
(II) At point, $[N_{2} O_{4}] = [N O_{2}] = 0.1 M Q = \frac{[N O_{2}]^{2}}{[N_{2} O_{4}]} = \frac{0.1 \times 0.1}{0.1} = 0.1 Q < K_{C}$
So, reaction proceeds from left to right
(III) Point D and F represent equilibrium because concentration is not changing with time.
So $K_{c} = Q$ at point [D and F]

Suggest Corrections

Similar questions

Q. 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.

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)

K_{c} = Q

, when point D or F is reached

N_{2} O_{4} ⇌ 2 N O_{3}, K_{C} = 4

. 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.

Q. When

0.5 m o l

N_{2} O_{4}

is placed in a

4.00 L

reaction vessel and heated at

400 K

79.3

% of the

N_{2} O_{4}

decomposes to

N O_{2}

. Calculate

K_{c}

and

K_{p}

400 K

for the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

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
NO $_{2}$ , are taken initially. Given: $Δ$ $_{f}$ G $^{\circ}$
(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.

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Reaction Quotient

Standard XI Chemistry

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