For the reaction, $N_{2} O_{4} (g) {⇌ K_{2}}^{K_{1}} 2 N O_{2} (g)$ , the rate of disappearance of $N O_{2}$ will be :

K_{1} [N_{2} O_{4}] - K_{2} [N O_{2}]^{2}

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2 K_{1} [N_{2} O_{4}] - 2 K_{2} [N O_{2}]^{2}

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K_{2} [N O_{2}]^{2} - K_{1} [N_{2} O_{4}]

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2 K_{2} [N O_{2}]^{2} - 2 K_{1} [N_{2} O_{4}]

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Solution

The correct option is A $K_{1} [N_{2} O_{4}] - K_{2} [N O_{2}]^{2}$
Rate of dissappearance of $N O_{2} i s r a t e o f f o r m a t i o n o f N_{2} O_{4}$
$K_{1} [N_{2} O_{4}$ ] = ${K_{2} [N O_{2}]}^{2}$

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N₂O₄ (g) ⇌ 2NO₂ (g)

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carried out at 298 K and 20 bar. Five moles of each of N $_{2}$ O $_{4}$ and
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For the elementary reaction 2A $⇌$ B,The forward and backward rate constants are $k_{1}$ and $k_{2}$ respectively. Then the rate of disappearance of A is equal to:

Q. Consider a system containing

N O_{2}

and

S O_{2}

in which

N O_{2}

is consumed in the following two parallel reactions:

2 N O_{2}_{1} N_{2} O_{4}

and

N O_{2} + S O_{2}_{2} N O + S O_{3}

. The rate of disappearance of

N O_{2}

will be equal to:

Q. In the reversible reaction

2 N O_{2}_{1} N_{2} O_{4}

, the rate of disappearance of

N O_{2}

is equal to:

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For the reaction, N2O4(g)⇌K2K12NO2(g), the rate of disappearance of NO2 will be :

The correct option is A K1[N2O4]−K2[NO2]2Rate of dissappearance of NO2israteofformationofN2O4K1[N2O4] =K2[NO2]2

For the reaction, $N_{2} O_{4} (g) {⇌ K_{2}}^{K_{1}} 2 N O_{2} (g)$ , the rate of disappearance of $N O_{2}$ will be :

The correct option is A $K_{1} [N_{2} O_{4}] - K_{2} [N O_{2}]^{2}$
Rate of dissappearance of $N O_{2} i s r a t e o f f o r m a t i o n o f N_{2} O_{4}$
$K_{1} [N_{2} O_{4}$ ] = ${K_{2} [N O_{2}]}^{2}$