You visited us 3 times! Enjoying our articles? Unlock Full Access!

Ideal Solutions

For the eleme...

Question

For the elementary reaction 2A $\to$ C ,the concentration of A after 30 minutes was found to be 0.01 mole/lit. If the rate constant of the reaction is $2.5 \times 10^{- 2}$ lit mole $^{- 1}$ sec $^{- 1}$ . The rate of the reaction at 30 minutes is:

2.5 \times 10^{- 4}

lit mole

^{- 1}

sec

^{- 1}

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

2.5 \times 10^{- 6}

lit mole

^{- 1}

sec

^{- 1}

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

2.5 \times 10^{- 2}

lit mole

^{- 1}

sec

^{- 1}

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

2.5 \times 10^{- 8}

lit mole

^{- 1}

sec

^{- 1}

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

Open in App

Solution

The correct option is B $2.5 \times 10^{- 6}$ lit mole $^{- 1}$ sec $^{- 1}$
Rate of Reaction = Rate Constant x ${[A]}^{2}$

$= 2.5 \times 10^{- 2} \times {[0.01]}^{2}$

$= 2.5 \times 10^{- 2} \times 10^{- 4}$

$= 2.5 \times 10^{- 6}$ lit mol $^{- 1}$ sec $^{- 1}$

Hence, the correct option is $B$

Suggest Corrections

Similar questions

Q. For the elementary reaction

2 A \to C

the concentration of

A

after 30 minutes was found to be 0.01 mole/lit. if the rate constant of the reaction is

2.5 \times 10^{- 2}

lit mole

{s e c}^{- 1}

the rate of the reaction at 30 minutes is:

Q. The specific rate of a reaction is

1.51 \times 10^{- 4}

lit mole

^{- 1}

sec

^{- 1}

. If the reaction is commenced with 0.2 mole lit

^{- 1}

of the reactant, the initial rate of the reaction in mole lit

^{- 1}

sec

^{- 1}

is:

Q. The rate constant

(K)

for the reaction

2 A + B \to

product, was found to be

2.5 \times 10^{- 5}

l i t r e m o l^{- 1} s e c^{- 1}

after

15 s e c

2.60 \times 10^{- 5} l i t m o l^{- 1} s e c^{- 1}

after

30 s e c

and

2.55 \times 10^{- 5}

l i t m o l^{- 1} s e c^{- 1}

after

50 s e c

. The order of reaction is:

Q. The decomposition of

{N H}_{3}

on platinum surface is zero order. What are the rate of production of

N_{2}

and

H_{2}

{m o l e . l i t}^{- 1} . {s e c}^{- 1}

K = 2.5 \times 10^{- 4} m o l e . l i t^{- 1} . {s e c}^{- 1}

K_{s p} o f A g C l

= 2.8 \times 10^{- 10}

25^{\circ}

C. Calculate solubility of AgCl in 0.1 (M) NaCl

Join BYJU'S Learning Program

For the elementary reaction 2A → C ,the concentration of A after 30 minutes was found to be 0.01 mole/lit. If the rate constant of the reaction is 2.5×10−2 lit mole−1 sec−1. The rate of the reaction at 30 minutes is:

The correct option is B 2.5×10−6 lit mole−1 sec−1Rate of Reaction = Rate Constant x [A]2 =2.5×10−2×[0.01]2=2.5×10−2×10−4=2.5×10−6 lit mol −1 sec−1Hence, the correct option is B

For the elementary reaction 2A $\to$ C ,the concentration of A after 30 minutes was found to be 0.01 mole/lit. If the rate constant of the reaction is $2.5 \times 10^{- 2}$ lit mole $^{- 1}$ sec $^{- 1}$ . The rate of the reaction at 30 minutes is:

The correct option is B $2.5 \times 10^{- 6}$ lit mole $^{- 1}$ sec $^{- 1}$
Rate of Reaction = Rate Constant x ${[A]}^{2}$

$= 2.5 \times 10^{- 2} \times {[0.01]}^{2}$

$= 2.5 \times 10^{- 2} \times 10^{- 4}$

$= 2.5 \times 10^{- 6}$ lit mol $^{- 1}$ sec $^{- 1}$

Hence, the correct option is $B$