25. For a reversible reaction where N2O4 converts to NO2 ,the rate of disappearance of NO2 will be 1.K1[N204]-k2[N02]2 2. 2K1[N204]-2k2[N02]2 3. K2[N02]2-k1[N204] 4. 2K2[NO2]2-2k1[N204]

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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. For a reaction,

N_{2} O_{5} ⟶ 2 N O_{2} + \frac{1}{2} O_{2}

Given:

\frac{- d [N_{2} O_{5}]}{d t} = k_{1} [N_{2} O_{5}]

\frac{d [N O_{2}]}{d t} = k_{2} [N_{2} O_{5}]

\frac{d [O_{2}]}{d t} = k_{3} [N_{2} O_{5}]

The relation between

k_{1}, k_{2}

and

k_{3}

are:

Q. For the reaction

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

- \frac{Δ [N_{2} O_{5}]}{Δ t} = k_{1} [N_{2} O_{5}], + \frac{[N O_{2}]}{Δ t} = k_{2} [N_{2} O_{5}], + \frac{Δ [O_{2}]}{Δ t} = k_{3} [N_{2} O_{5}]

Thus,

Q. For the reaction :

N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2} \frac{- d [N_{2} O_{5}]}{d t} = K_{1} [N_{2} O_{5}], \frac{d [N O_{2}]}{d t} = K_{2} [N_{2} O_{5}], a n d \frac{d [O_{2}]}{d t} = K_{3} [N_{2} O_{5}]

The

K_{1}, K_{2}

and

K_{3}

are related as :

Q. 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 :

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