MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Order of Reaction

For a certain...

Question

For a certain reaction the rate law is rate $= k [C]^{3 / 2}$ . If the rate of the reaction is $0.020$ mol L $^{- 1}$ s $^{- 1}$ when $[C]$ = $1.0$ M, what is the rate when $[C]$ = $0.60$ M?

A

0.0093

mol L

^{- 1}

s

^{- 1}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

B

0.012

mol L

^{- 1}

s

^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

0.033

mol L

^{- 1}

s

^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

0.040

mol L

^{- 1}

s

^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $0.0093$ mol L $^{- 1}$ s $^{- 1}$
The rate law is rate $= k [C]^{3 / 2}$
The rate of the reaction is $0.020 m o l L^{- 1} s^{- 1}$ when $[C] = 1.0$ M.
The rate law becomes $0.020 m o l L^{- 1} s^{- 1} = k [1.0 M]^{3 / 2}$
$\Rightarrow k = 0.020 m o l^{- 0.5} L^{0.5} s^{- 1}$
When, $[C] = 0.60 M$ , the rate law is
Rate $= k [C]^{3 / 2}$
Rate $= (0.020 m o l^{- 0.5} L^{0.5} s^{- 1}) \times [0.60 M]^{3 / 2}$
Rate $= 0.0093 m o l L^{- 1} s^{- 1}$

Suggest Corrections

thumbs-up

0

Similar questions

Q. For the reaction 2A + B + C

\to A_{2} B

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

^{2}

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 a reaction

2 A + B \to P,

when concentration of B alone is doubled,

t_{\frac{1}{2}}

does not change and when concentrations of both A and B is doubled, rate increases by a factor of 4. The unit of rate constant is,

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 $0.06 m o l L^{- 1}$ .

t_{1 / 2} v / s [R]_{0}

for a reaction is a straight-line parallel to x-axis. The unit for the rate constant of this reaction is:

Q. For the reaction:

2 A + B \to A_{2} B

= k [A] [B]^{2}

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

Calculate the initial rate of the 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]

0.06 m o l L^{- 1}

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Order and Molecularity of Reaction

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Order of Reaction

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon