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

Byju's Answer

Standard XII

Chemistry

Vant Hoff's Equation and Effect of Temperature on Equilibrium Constant

Use the exper...

Question

Use the experimental data in the table to determine the rate law for this reaction, $A + B ⟶ A B$ .
These data were obtained when the reaction was studied:
$[A]$ $[B]$ $\frac{Δ [A B]}{Δ t} |_{t = 0}$ $m o l$ $L^{- 1} {s e c}^{- 1}$
$0.1 M$ $0.1 M$ $2 \times 10^{- 4}$
$0.2 M$ $0.1 M$ $2 \times 10^{- 4}$
$0.3 M$ $0.3 M$ $1.8 \times 10^{- 3}$
What is the rate equation for the reaction?

Rate

= k [A] [B]

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

Rate

= k {[A]}^{2}

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

Rate

= k [B]

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

Rate

= k {[B]}^{2}

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

Open in App

Solution

The correct option is D Rate $= k {[B]}^{2}$
Let the rate be given by $\frac{d A B}{d t} = k [A]^{x} [B]^{y}$
where order of the reaction=x+y
Substituting given date,
$2 \times 10^{- 4} = k (0.1)^{x} (0.1)^{y}$ -(1)
$2 \times 10^{- 4} = k (0.2)^{x} (0.1)^{y}$ -(2)
$1.8 \times 10^{- 3} = k (0.3)^{x} (0.3)^{y}$ -(3)
From (1)and (2), $(\frac{0.1}{0.2})^{x} = 1 => x = 0$
From (2) and (3), $\frac{2}{18} = (\frac{1}{3})^{y} => y = 2$
Rate= $k [B]^{2}$

Suggest Corrections

Similar questions

For the non - stoichiometric reaction, 2A+B $\to$ C + D, the following kinetic data were obtained in three separate experiments, all at 298 K.

$\begin{matrix} Initial & Initial & Initial rate of concentration & concentration & formation of C [A] & [B] & (m o l L^{- 1} s^{- 1}) (i) & 0.1 M & 0.1 M & 1.2 \times 10^{- 3} (i i) & 0.1 M & 0.2 M & 1.2 \times 1^{- 3} (i i i) & 0.2 M & 0.1 M & 2.4 \times 10^{- 3} \end{matrix}$ The rate law for the formation of C is

Q. For a reaction

A + 2 B \to C + D

, the following data were obtained

The correct rate law expression will be

Q. For the non-stoichiometric reaction,

2 A + B ⟶ C + D

, the following kinetic data were obtained in three separate experiments, all at

298 K

Initial Concentration $[A]$	Initial Concentration $[B]$	Initial rate of formation of $C$ $(m o l L^{- 1} s^{- 1})$
$0.1 M$	$0.1 M$	$1.2 \times 10^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 10^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 10^{- 3}$

The rate law for the formation of

C

is:

Q. For a reaction between

A

and

B

, the initial rate of reaction is measured for various initial concentrations of

A

and

B

. The data provided are:

Expt. No.	$[A]$	$[B]$	Initial reaction rate $(m o l L^{- 1} s^{- 1})$
$1.$	$0.2 M$	$0.3 M$	$5 \times 10^{- 5}$
$2.$	$0.2 M$	$0.1 M$	$5 \times 10^{- 5}$
$3.$	$0.4 M$	$0.05 M$	$7.5 \times 10^{- 5}$

The overall order of the reaction is:

Q. For the non-stoichiometre reaction

2 A + B \to C + D

, the following kinetic data were obtained in three separate experiments, all at

298 K

Initial Concentration $(A)$	Initial Concentration $(B)$	Initial rate of formation of $C$ $(m o l L^{-} S^{-})$
$0.1 M$	$0.1 M$	$1.2 \times 10^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 10^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 10^{- 3}$

The rate law for the formation of

C

is__________.

Join BYJU'S Learning Program

$[A]$	$[B]$	$\frac{Δ [A B]}{Δ t} \|_{t = 0}$ $m o l$ $L^{- 1} {s e c}^{- 1}$
$0.1 M$	$0.1 M$	$2 \times 10^{- 4}$
$0.2 M$	$0.1 M$	$2 \times 10^{- 4}$
$0.3 M$	$0.3 M$	$1.8 \times 10^{- 3}$

Use the experimental data in the table to determine the rate law for this reaction, A+B⟶AB.These data were obtained when the reaction was studied:[A][B]Δ[AB]Δt|t=0 mol L−1sec−10.1M0.1M2×10−40.2M0.1M2×10−40.3M0.3M1.8×10−3What is the rate equation for the reaction?

The correct option is D Rate =k[B]2Let the rate be given by dABdt=k[A]x[B]ywhere order of the reaction=x+ySubstituting given date,2×10−4=k(0.1)x(0.1)y-(1)2×10−4=k(0.2)x(0.1)y-(2)1.8×10−3=k(0.3)x(0.3)y-(3)From (1)and (2), (0.10.2)x=1=>x=0From (2) and (3), 218=(13)y=>y=2Rate= k[B]2