The unit of rate constant for the reaction 2H2 -2NO- 2H2O - N2 which hasRate - K-H2-NO-2- is-

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Standard XII

Chemistry

Law of Mass Action

The unit of r...

Question

The unit of rate constant for the reaction $2 H_{2} + 2 NO \to 2 H_{2} O + N_{2}$ which has
Rate $= K [H_{2}] [N O]^{2},$ is:

{mol L}^{- 1} s^{- 1}

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s^{- 1}

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{mol}^{- 2} L^{2} s^{- 1}

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{mol}^{- 1} L^{1} s^{- 1}

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Solution

The correct option is C ${mol}^{- 2} L^{2} s^{- 1}$
Unit of rate constant $(k)$ for a $n^{t h}$ order reaction is $= {mol}^{1 - n} L^{n - 1} s^{- 1}$
Order of a reaction is the sum of powers of concentration terms in rate law equation.
Here order = $2 + 1 = 3$
So unit of $k = {mol}^{- 2} L^{2} s^{- 1}$

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Similar questions

Q. The unit of rate constant for the reaction,

2 H_{2} + 2 N O \to 2 H_{2} O + N_{2}

which has

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

, is:

Q. For the reaction,

2 H_{2} + 2 N O \to N_{2} + 2 H_{2} O

the following mechanism has been proposed:-

2 N O ⇌ N_{2} O_{2}

; equilibrium constant

K_{1} (f a s t)

ii)

N_{2} O_{2} + H_{2}_{2} N_{2} O + H_{2} O (s l o w)

iii)

N_{2} O + H_{2} \to N_{2} + H_{2} O (f a s t)

What will be the rate law of this reaction?

The possible mechanism for the reaction:

$2 H_{2 +} 2 N O \to N_{2} + 2 H_{2} O$ is

$(i) 2 N O ⇌ N_{2} O_{2} (i i) N_{2} O_{2} + H_{2} \to N_{2} O + H_{2} O (slow) (i i i) N_{2} O + H_{2} \to N_{2} H_{2} O (fast)$ What is (i) the rate law for the reaction (ii) the order of the reaction?

Q. For the reaction

2 H_{2} + 2 N O \to N_{2} + 2 H_{2} O

, the following mechanism has been suggested :

2 N O ⇌ N_{2} O_{2}

equilibrium constant

k_{1}

(fast)

N_{2} O_{2} + H_{2}_{2} N_{2} O + H_{2} O (s l o w)

N_{2} O + H_{2}_{3} N_{2} + H_{2} O (f a s t)

Establish the rate law for given reaction.

Q. For the reaction:

2 H_{2} + 2 N O ⇌ 2 H_{2} O + N_{2}

, the following rate data was obtained:

S. No.	$[N O]$ $m o l$ $L^{- 1}$	$[H_{2}]$ $m o l$ $L^{- 1}$	Rate: $m o l$ $L^{- 1}$ ${s e c}^{- 1}$
$1$	$0.40$	$0.40$	$4.6 \times 10^{- 3}$
$2$	$0.80$	$0.40$	$18.4 \times 10^{- 3}$
$3$	$0.40$	$0.80$	$9.2 \times 10^{- 3}$

Calculate the following:
(1) The overall order of reaction.
(2) The rate law.
(3) The value of rate constant

(k)

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The unit of rate constant for the reaction 2H2+2NO→2H2O+N2 which has Rate =K[H2][NO]2, is:

The correct option is C mol−2 L2 s−1Unit of rate constant (k) for a nth order reaction is = mol1−n Ln−1 s−1 Order of a reaction is the sum of powers of concentration terms in rate law equation. Here order = 2+1=3 So unit of k= mol−2 L2 s−1

The unit of rate constant for the reaction $2 H_{2} + 2 NO \to 2 H_{2} O + N_{2}$ which has
Rate $= K [H_{2}] [N O]^{2},$ is: