Following reaction can take place in both direction A k 1 k 2 - B- It is given that for the forward reaction -B-Rate 0-01 M 1 - 10-2 Ms-1 0-02 M 2 - 10-2 Ms-1Hence - net reaction rate of B is -

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

Byju's Answer

Standard XII

Chemistry

Rate of Reaction

Following rea...

Question

Following reaction can take place in both direction $A_{1} B$ , It is given that for the forward reaction :
[B] Rate
$0.01 M$ $1 \times 10^{- 2} M s^{- 1}$
$0.02 M$ $2 \times 10^{- 2} M s^{- 1}$
Hence , net reaction rate of B is :

k_{1}

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

k_{1} - k_{2}

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

k_{1} [A] - k_{2}

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

none of these

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

Open in App

Solution

The correct option is A $k_{1}$
From the graph, it is clear that the Following reaction is a Zero Order Reaction.

So, Rate = Rate Constant = $k_{1}$

Suggest Corrections

Similar questions

For the elementary reaction 2A $⇌$ B,The forward and backward rate constants are $k_{1}$ and $k_{2}$ respectively. Then the rate of disappearance of A is equal to:

Q. A reaction can take place by two paths.

k_{1}

and

k_{2}

are rate constants for the two paths &

E_{1}

and

E_{2}

are their respective activation energies.
At temperature

T_{a} : k_{1} > k_{2}, E_{1} < E_{2}

Its temperature is raised to

T_{b}

, the rate constants change to

k_{1}^{'}

k_{2}^{'}

. Which relation is correct between

k_{1}, k_{2}, k_{1}^{'}

k_{2}^{'}

(considering activation energy does not change with temperature)?

Q. In the sequence of reaction:

A_{1} B_{2} C_{3} D, k_{3} > k_{2} > k_{1}

then the rate determining step of the reaction is:

Q. For the given reaction,

A_{1} K_{2} B

Where

K_{1}

is zero order rate constant and

K_{2}

is first rate constant. The concentration of

B

at any time can be given by the experssion:

Q. For gaseous reaction, following data is given:

A \to B, k_{1} = 10^{15} e^{- 2000 / T}

C \to D, k_{2} = 10^{14} e^{- 1000 / T}

The temperature at which

k_{1} = k_{2}

is:

Join BYJU'S Learning Program

[B]	Rate
$0.01 M$	$1 \times 10^{- 2} M s^{- 1}$
$0.02 M$	$2 \times 10^{- 2} M s^{- 1}$

Following reaction can take place in both direction Ak1⇌k2B, It is given that for the forward reaction :[B]Rate0.01M1×10−2Ms−10.02M2×10−2Ms−1Hence , net reaction rate of B is :

The correct option is A k1From the graph, it is clear that the Following reaction is a Zero Order Reaction.So, Rate = Rate Constant = k1

Following reaction can take place in both direction $A_{1} B$ , It is given that for the forward reaction :
[B] Rate
$0.01 M$ $1 \times 10^{- 2} M s^{- 1}$
$0.02 M$ $2 \times 10^{- 2} M s^{- 1}$
Hence , net reaction rate of B is :

The correct option is A $k_{1}$
From the graph, it is clear that the Following reaction is a Zero Order Reaction.

So, Rate = Rate Constant = $k_{1}$