The unit of rate constant for the reaction- 2H2 - 2NO - 2H2O - N2which has rate - k-H2-NO-2- is-

The correct option is C mol^ 2 L^2 s^ 1 Unit of rate constant for the reaction is k = rate[H_2][NO]^2 = mol L^ 1 s^ 1(mol L^ 1)(mol L^ 1)^2 = mol^ 2 L ...

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Byju's Answer

Standard XII

Chemistry

Order of Reaction

The unit of r...

Question

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:

m o l L^{- 1} s^{- 1}

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s^{- 1}

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m o l^{- 2} L^{2} s^{- 1}

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m o l L^{- 1}

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Solution

The correct option is C $m o l^{- 2} L^{2} s^{- 1}$
Unit of rate constant for the reaction is
$k = \frac{r a t e}{[H_{2}] [N O]^{2}} = \frac{m o l L^{- 1} s^{- 1}}{(m o l L^{- 1}) (m o l L^{- 1})^{2}} = m o l^{- 2} L^{2} s^{- 1}$ .

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Similar questions

Q. For the reaction,

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

, the following kinetic data were obtained:

Expt. No.	$[H_{2}]$ $(m o l L^{- 1})$	$[N O]$ $(m o l L^{- 1})$	Rate of reaction $(m o l L^{- 1} s^{- 1})$
$1.$	$0.12$	$0.12$	$0.25 \times 10^{- 4}$
$2.$	$0.12$	$0.24$	$1.0 \times 10^{- 4}$
$3.$	$0.24$	$0.24$	$2.0 \times 10^{- 4}$

Determine the rate law and the rate constant.

Q. 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:

Q. For the reaction 2A + B + C

\to A_{2} B

+ C the rate law is found to be Rate =k[A][B]

^{2}

with

k = 2 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

The initial rate of reaction with

[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1} a n d [C] = 0.8 m o l L^{- 1}

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)

For the reaction, $N_{2} O_{5} (g) \to N O_{2} (g) + \frac{1}{2} O_{2} (g)$ The value of rate of disappearance of $N_{2} O_{5}$ is given as $6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1} .$ The rate of formation of $N O_{2}$ and $O_{2}$ is given respectively as:

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The unit of rate constant for the reaction, 2H2+2NO→2H2O+N2which has rate=k[H2][NO]2, is:

The correct option is C mol−2L2s−1Unit of rate constant for the reaction isk=rate[H2][NO]2=mol L−1s−1(mol L−1)(mol L−1)2=mol−2L2s−1.

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:

The correct option is C $m o l^{- 2} L^{2} s^{- 1}$
Unit of rate constant for the reaction is
$k = \frac{r a t e}{[H_{2}] [N O]^{2}} = \frac{m o l L^{- 1} s^{- 1}}{(m o l L^{- 1}) (m o l L^{- 1})^{2}} = m o l^{- 2} L^{2} s^{- 1}$ .