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Standard XII

Chemistry

Arrhenius Equation

Trial 1 Trial...

Question

Trial 1 Trial 2
[A] (mol/L) Rate [A](mol/L) Rate
0.10 0.6 0.10 0.9
0.20 0.6 0.20 0.9
0.30 0.6 0.30 0.9
0.40 0.6 0.40 0.9
Consider the following chemical reaction and experimental data:
$A (a q) \to B (a q) + C (g)$
(A) What is the rate expression for trial $1$ ?
(B) What is the rate constant for trial $1$ ?

A. rate

= k {[A]}_{2} = k

; B.

k = 0.2

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A. rate

= k {[A]}_{1} = k

; B.

k = 0.9

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A. rate

= k {[A]}_{0} = k

; B.

k = 0.6

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None of the above.

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Solution

The correct option is D A. rate $= k {[A]}_{0} = k$ ; B. $k = 0.6$
$A \to B \to C$
(A) Rate expression for trial 1
$R_{1} = K_{1} [A]_{0}$
Therefore Rate= $K_{1} [0.10]$
Rate = $0.6 [0.10]$
(B) Rate constant for trial 1 is $K_{1} = 0.6$

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Similar questions

For reaction: A + B $\to$ Products, the rate if the reaction at various concentration are given below:

$\begin{matrix} Expt. No. & (A) & (B) & Rate 1 & 0.2 & 0.2 & 2 2 & 0.2 & 0.4 & 4 3 & 0.6 & 0.4 & 36 \end{matrix}$

Q. For the reaction

2 A + B \to C

, the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is:

$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	$Initial Rate (m o l L^{- 1} s^{- 1})$
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

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

Q. For the hypothetical reaction,

2 A + B ⟶

Products, the following data are obtained:

Expt. No.	Initial conc. of $(A)$ $(m o l L^{- 1})$	Initial conc. of $(B)$ $(m o l L^{- 1})$	Initial rate $m o l$ $L^{- 1}$ $s^{- 1}$
$1.$	$0.10$	$0.20$	$3 \times 10^{2}$
$2.$	$0.30$	$0.40$	$3.6 \times 10^{3}$
$3.$	$0.30$	$0.80$	$1.44 \times 10^{4}$
$4.$	$0.10$	$0.40$	______
$5.$	$0.20$	$0.60$	______
$6.$	$0.30$	$1.20$	______

Find out how the rate of the reaction depends upon the concentration of

A

and

B

and fill in the blanks.

Q. 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 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]

is reduced to

0.06 m o l L^{- 1}

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Trial 1		Trial 2
[A] (mol/L)	Rate	[A](mol/L)	Rate
0.10	0.6	0.10	0.9
0.20	0.6	0.20	0.9
0.30	0.6	0.30	0.9
0.40	0.6	0.40	0.9

Trial 1 Trial 2 [A] (mol/L) Rate [A](mol/L) Rate 0.10 0.6 0.10 0.9 0.20 0.6 0.20 0.9 0.30 0.6 0.30 0.9 0.40 0.6 0.40 0.9 Consider the following chemical reaction and experimental data: A(aq)→B(aq)+C(g)(A) What is the rate expression for trial 1?(B) What is the rate constant for trial 1?

The correct option is D A. rate =k[A]0=k; B. k=0.6A→B→C(A) Rate expression for trial 1R1=K1[A]0Therefore Rate= K1[0.10]Rate = 0.6[0.10](B) Rate constant for trial 1 is K1=0.6

The correct option is D A. rate $= k {[A]}_{0} = k$ ; B. $k = 0.6$
$A \to B \to C$
(A) Rate expression for trial 1
$R_{1} = K_{1} [A]_{0}$
Therefore Rate= $K_{1} [0.10]$
Rate = $0.6 [0.10]$
(B) Rate constant for trial 1 is $K_{1} = 0.6$