Match the rate expressions in LIST-I for the decomposition of NH3 with the corresponding profiles provided in LIST-II.1, k and k1 are constants having appropriate units. LIST-I LIST-II(I)rate=k[NH3]1+k1[NH3]under all possible initial concentrationsof NH3 (P) (II)rate=k[NH3]1+k1[NH3]under high initial concentrations of NH3 such that k1NH3>>1(Q) (III) rate=k[NH3]1+k1[NH3]NH3under high initial concentrations of such that k1[NH3]<<1 (R)(IV)rate=k[NH3]21+k1[NH3]under low initial concentrations of NH3 such that k1[NH3]<<1 (S) (T)

I - At low concentrations of NH3 - first order At high concentrations of NH3 - 2nd orderII - when k1[NH3]>>1 , it follows zero order kineticsrate=k[NH3]k1[NH3]=constantIII – when k1[NH3]<<1 , it follows first order kineticsrate=k[NH3] IV - rate=k[NH3]21+k1[NH3] When k1[NH3]<<1 , it follows 2nd order kineticsrate=k[NH3]2

Match the rate expressions in LIST-I for the decomposition of NH3 with the corresponding profiles provided in LIST-II.1, k and k1 are constants having appropriate units. LIST-I LIST-II(I)rate=k[NH3]1+k1[NH3]under all possible initial concentrationsof NH3 (P) (II)rate=k[NH3]1+k1[NH3]under high initial concentrations of NH3 such that k1NH3>>1(Q) (III) rate=k[NH3]1+k1[NH3]NH3under high initial concentrations of such that k1[NH3]<<1 (R)(IV)rate=k[NH3]21+k1[NH3]under low initial concentrations of NH3 such that k1[NH3]<<1 (S) (T)

I - At low concentrations of NH3 - first order At high concentrations of NH3 - 2nd orderII - when k1[NH3]>>1 , it follows zero order kineticsrate=k[NH3]k1[NH3]=constantIII – when k1[NH3]<<1 , it follows first order kineticsrate=k[NH3] IV - rate=k[NH3]21+k1[NH3] When k1[NH3]<<1 , it follows 2nd order kineticsrate=k[NH3]2

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Match the rate expressions in LIST-I for the decomposition of NH3 with the corresponding
profiles provided in LIST-II.1, k and $k_{1}$ are constants having appropriate units.
LIST-I LIST-II
(I) $r a t e = \frac{k [N H_{3}]}{1 + k_{1} [N H_{3}]}$ under all possible initial concentrationsof $N H_{3}$ (P)

(II) $r a t e = \frac{k [N H_{3}]}{1 + k_{1} [N H_{3}]}$ under high initial concentrations of $N H_{3}$ such that $k_{1} [N H_{3}] > > 1$ (Q)

(III) $r a t e = \frac{k [N H_{3}]}{1 + k_{1} [N H_{3}]}$ $N H_{3}$ under high initial concentrations of such that $k_{1} [N H_{3}] < < 1$ (R)
(IV) $r a t e = \frac{k {[N H_{3}]}^{2}}{1 + k_{1} [N H_{3}]}$ under low initial concentrations of $N H_{3}$ such that $k_{1} [N H 3] < < 1$ (S)

(T)

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$I \to R, II \to T, III \to P, IV - Q$

$I \to R, II \to P, III \to T, IV - Q$

$I \to S, II \to P, III \to Q, IV - T$

$I \to T, II \to S, III \to P, IV - R$

answer is B.

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Detailed Solution

I - At low concentrations of $N H_{3}$ - first order
At high concentrations of $N H_{3}$ - 2nd order
II - when $k_{1} [N H_{3}] > > 1$ , it follows zero order kinetics

$r a t e = \frac{k [N H_{3}]}{k_{1} [N H_{3}]} = constant$

III – when $k_{1} [N H_{3}] < < 1$ , it follows first order kinetics

$r a t e = k [N H_{3}]$
IV - $r a t e = \frac{k {[N H_{3}]}^{2}}{1 + k_{1} [N H_{3}]}$
When $k_{1} [N H_{3}] < < 1$ , it follows 2nd order kinetics

$r a t e = k {[N H_{3}]}^{2}$

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