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Byju's Answer

Standard XII

Chemistry

Order of Reaction

C Cl 3 CHO+NO...

Question

$C {C l}_{3} C H O + N O ⟶ C H {C l}_{3} + N O + C O$
The rate of the reaction above is equal to rate $= k [C {C l}_{3} C H O] [N O]$ .

If the concentration is expressed in mol L $^{- 1}$ , find the unit of $k$ ?

L mol

^{- 1}

^{- 1}

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mol L

^{- 1}

^{- 1}

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^{2}

mol

^{- 2}

^{- 1}

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^{- 1}

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Solution

The correct option is A L mol $^{- 1}$ s $^{- 1}$
Rate $= \frac{d x}{d t} = k [C {C l}_{3} C H O] [N O]$

$k = \frac{d x}{d t \times k [C {C l}_{3} C H O] [N O]}$

$= \frac{m o l L^{- 1}}{s^{- 1} \times m o l L^{- 1} \times m o l L^{- 1}}$

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

Hence, the correct option is $A$

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Similar questions

Q. The rate of the reaction,

C {C l}_{3} C H O + N O ⟶ C H {C l}_{3} + N O + C O

, is given by the equation, rate

= k [C {C l}_{3} C H O] [N O]

. If concentration is expressed in

m o l / l i t r e

, the unit of

k

is:

Q. The rate of the reaction,

2 N O + O_{2} ⟶ 2 N O_{2}

, at

25^{o} C

0.028

m o l

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

. The experimental rate is given by,

r = k {[N O]}^{2} [O_{2}]

.
If the initial concentrations of the reactants are

O_{2} = 0.040

m o l

L^{- 1}

and

N O = 0.01

m o l

L^{- 1}

, the rate constant of the reaction is:

Q. The reaction

2 N O + O_{2} \to 2 N O_{2}

, follows the rate law

= k {[N O]}^{2} [O_{2}]

. What is the order of the reaction? If

k = 2.0 \times 10^{- 6} {m o l}^{- 2} L^{2} s^{- 1}

, what is the rate of the reaction when

[N O] = 0.04

m o l

L^{- 1}

and

[O_{2}] = 0.2

m o l

L^{- 1}

Q. In a catalytic conversion of

N_{2}

N H_{3}

by Haber's process, the rate of reaction was expressed as change in the concentration of ammonia per time is

40 \times 10^{- 3}

mol L

^{- 1}

^{- 1}

. If there is no side reaction, the rate of the reaction as expressed in terms of hydrogen is :

(in mol L

^{- 1}

^{- 1}

)

For the reaction, $2 A + B \to A_{2} B$ the rate $= k [A] [B]^{2}$ with $k = 2.0 \times 10^{- 6} m o l^{- 2} L^{- 2} s^{- 1}$ . Calculate the initial rate of reaction when $[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1}$ . Calculate the rate of reaction after [A] is reduced to $0.06 m o l L^{- 1}$ .

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CCl3CHO+NO⟶CHCl3+NO+COThe rate of the reaction above is equal to rate =k[CCl3CHO][NO]. If the concentration is expressed in mol L −1, find the unit of k?

The correct option is A L mol −1 s −1Rate =dxdt=k[CCl3CHO][NO]k=dxdt×k[CCl3CHO][NO]=molL−1s−1×molL−1×molL−1=Lmol−1s−1Hence, the correct option is A

$C {C l}_{3} C H O + N O ⟶ C H {C l}_{3} + N O + C O$
The rate of the reaction above is equal to rate $= k [C {C l}_{3} C H O] [N O]$ .

If the concentration is expressed in mol L $^{- 1}$ , find the unit of $k$ ?