Match List-I with List-II
|
List-I Rate expression |
List-II Overall order of reaction |
|
(A) \( r = k[A]^{0.2}[B]^{0.3} [C] \) |
(I) 3/10 |
|
(B) \( r = k[A]^{0.2}[B]^{-0.3} [C] \) |
(II) 1 |
|
(C) \( r = k[A][B]^{0.3} [C]^{-1} \) |
(III) 3/2 |
|
(D) \( r = k[A]^{0.2}[B]^{0.3} [C]^{0.5} \) |
(IV) 9/10 |
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 4
The correct answer is Option (4) → (A)-(III), (B)-(IV), (C)-(I), (D)-(II)
The order of a reaction is the sum of the powers of the concentration terms in the rate law. The powers are found by experiment, so they can be fractions, zero or even negative.
(A) \(r = k[A]^{0.2}[B]^{0.3} [C]\) — This matches (III) 3/2. 0.2 + 0.3 + 1 = 1.5 = 3/2.
(B) \(r = k[A]^{0.2}[B]^{-0.3} [C]\) — This matches (IV) 9/10. The negative power is subtracted: 0.2 − 0.3 + 1 = 0.9 = 9/10.
(C) \(r = k[A][B]^{0.3} [C]^{-1}\) — This matches (I) 3/10. 1 + 0.3 − 1 = 0.3 = 3/10.
(D) \(r = k[A]^{0.2}[B]^{0.3} [C]^{0.5}\) — This matches (II) 1. 0.2 + 0.3 + 0.5 = 1.
Shortcut: (C) gives 1 + 0.3 − 1 = 3/10, and (C)-(I) appears only in Option (4).