Consider a system containing NO2 and SO2 in which NO2 is consumed in the following two parallel reactions- 2NO2k1- N2O4 and NO2 - SO2 k2- NO-SO3- The rate of disappearance of NO2 will be equal to-

The correct option is D 2k_1[NO_2]^2+k_2[NO_2][SO_2] For the reaction 2NO_2k_1→ N_2O_4 and #160; NO_2 + SO_2 k_2→ NO+SO_3 , the rate of the re ...

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Byju's Answer

Standard XII

Chemistry

Reaction Quotient

Consider a sy...

Question

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:

k_{1} [N O_{2}]^{2} + k_{2} [N O_{2}]

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k_{1} [N O_{2}]^{2} + k_{2} [N O_{2}] [S O_{2}]

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2 k_{1} [N O_{2}]^{2}

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2 k_{1} [N O_{2}]^{2} + k_{2} [N O_{2}] [S O_{2}]

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Solution

The correct option is D $2 k_{1} [N O_{2}]^{2} + k_{2} [N O_{2}] [S O_{2}]$
For the reaction $2 N O_{2}_{1} N_{2} O_{4}$ and $N O_{2} + S O_{2}_{2} N O + S O_{3}$ , the rate of the reaction is $- \frac{1}{2} \frac{d [N O_{2}]}{d t} = k_{1} [N O_{2}]^{2} .$
$⟹$ $- \frac{d [N O_{2}]}{d t} = 2 k_{1} [N O_{2}]^{2}$ .....(1)

For the reaction $2 N O 2_{1} N_{2} O_{4}$ and $N O_{2} + S O_{2}_{2} N O + S O_{3}$ , the rate of the reaction is $- \frac{d [N O_{2}]}{d t} = k_{2} [N O_{2}] [S O_{2}]$ ......(2)
So, from equations (1) and (2), we get the rate of disappearance of $N O_{2}$ is equal to $- \frac{d [N O_{2}]}{d t} = 2 k_{1} [N O_{2}]^{2} + k_{2} [N O_{2}] [S O_{2}] .$

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Similar questions

Q. The decreasing order of

N - O

bond lengths in

N O_{2}^{+}

N O_{2}^{-}

and

N O_{3}^{-}

is:

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?

N₂O₄ (g) ⇌ 2NO₂ (g)

Q. Arrange

N O_{2}^{+}, N O_{2}^{-}

and

N O_{3}^{-}

in the decreasing order of their

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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. 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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Consider a system containing NO2 and SO2 in which NO2 is consumed in the following two parallel reactions: 2NO2k1→N2O4 and NO2+SO2k2→NO+SO3. The rate of disappearance of NO2 will be equal to:

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: