The rate expression for the reaction $A (g) + B (g) \to C (g) is k C_{A}^{2} C_{B}^{1 / 2}$ . What changes in the initial concentration of $A$ and $B$ will cause the rate of reaction increase by a factor of eight:

C_{A} \times 2; C_{B} \times 2

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

C_{A} \times 2; C_{B} \times 4

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

C_{A} \times 1; C_{B} \times 4

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

C_{A} \times 4; C_{B} \times 1

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

Open in App

Solution

The correct option is B $C_{A} \times 2; C_{B} \times 4$
Given,
$A (g) + B (g) \to C (g)$

$Rate expression = k C_{A}^{2} C_{B}^{1 / 2}$
$When concentration of A increases 2 times \to [2 C_{A}] When concentration of B increases 4 times \to [4 C_{B}]$

$New rate = k [2 C_{A}]^{2} [4 C_{B}]^{1 / 2}$

$= 4 \times 2 k [C_{A}]^{2} [C_{B}]^{1 / 2}$

$New rate = 8 k [C_{A}]^{2} [C_{B}]^{1 / 2}$

So, the new rate of reaction increased by factor eight.
In this case correct option is B.

Suggest Corrections

Similar questions

Q. The rate expression for reaction

A (g) + B (g) ⟶ C (g)

is rate

= k {[A]}^{1 / 2} {[B]}^{2}

. What change in rate if initial concentration of A and B increase by factor 4 and 2 respectively?

If a reaction has the experimental rate expression rate = $K [A]^{2} [B]$ , if the concentration of A is doubled and the concentration of B is halved, the what happens to the reaction rate:-

Q. For a reaction

A_{(g)} \to B_{(g)} + C_{(g)}

, the rate constant for the reaction is

3 \times 10^{- 3} M^{-} m i n^{- 1}

. At what concentration of A will at the rate of reaction be

2 \times 10^{- 3}

M min.

Q. For a hypothetical reaction

A ⟶ B

,it is found that the rate constant=

x s^{- 1}

.By what factor the rate is increase if the initial concentration of

A

is tripled?

Q. In the reaction,

A ⟶ B

, when the initial concentration of reactant is halved, the half-life increases by a factor of eight, what will be the order of the reaction?

Join BYJU'S Learning Program

The rate expression for the reaction A(g)+B(g)→C(g) is kC2A C1/2B. What changes in the initial concentration of A and B will cause the rate of reaction increase by a factor of eight:

The rate expression for the reaction $A (g) + B (g) \to C (g) is k C_{A}^{2} C_{B}^{1 / 2}$ . What changes in the initial concentration of $A$ and $B$ will cause the rate of reaction increase by a factor of eight: