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Standard XII

Chemistry

Order of Reaction

Find the valu...

Question

Find the values of A, B and C in the following table for the reaction :

$X + Y ⟶ Z$

The reaction is first order with respect to $X$ and zero order with respect to $Y$

$E x p$ $[X] (m o l L^{- 1})$ $[Y] (m o l L^{- 1})$
$I n i t i a l r a t e (m o l L^{- 1} s - 1)$
1. $0.1$ $0.1$ $2 \times 10^{- 2}$
2. $A$ $0.2$ $4 \times 10^{- 2}$
3. $0.4$ $0.4$ $B$
4. $C$ $0.2$ $2 \times 10^{- 2}$

A = 0.2 m o l L^{- 1}, B = 8 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.1 m o l L^{- 1}

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A = 0.4 m o l L^{- 1}, B = 4 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.2 m o l L^{- 1}

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A = 0.2 m o l L^{- 1}, B = 2 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.4 m o l L^{- 1}

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A = 0.4 m o l L^{- 1}, B = 2 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.4 m o l L^{- 1}

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Solution

The correct option is A $A = 0.2 m o l L^{- 1}, B = 8 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.1 m o l L^{- 1}$

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Similar questions

Q. For the reaction 2A + B + C

\to A_{2} B

+ C the rate law is found to be Rate =k[A][B]

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with

k = 2 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

The initial rate of reaction with

[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1} a n d [C] = 0.8 m o l L^{- 1}

Q. Fill in the blanks in the following table which treats reaction of a compound

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with a compound

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, that is of the first-order with respect to

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and zero-order with respect to

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Expt. No.	$[A]$ $(m o l L^{- 1})$	$[B]$ $(m o l L^{- 1})$	Initial rate $(m o l L^{- 1} s^{- 1})$
$1.$	$0.1$	$0.1$	$2.0 \times 10^{- 2}$
$2.$	___	$0.2$	$4.0 \times 10^{- 2}$
$3.$	$0.4$	$0.4$	___
$4.$	___	$0.2$	$2.0 \times 10^{- 2}$

At 27°C and 37°C the rates of a reaction are given as 1.6*10^-2 mol L^-1s^-1 and 3.2*10^-2 mol L^-1s^-1.Calculate the energy of activation for the give reaction.

The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

Experiment	A/ mol L⁻¹	B/ mol L⁻¹	Initial rate/mol L⁻¹ min⁻¹
I	0.1	0.1	2.0 × 10⁻²
II	--	0.2	4.0 × 10⁻²
III	0.4	0.4	--
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Q. Rate For the reaction

A + B \to p r o d u c t s

, what will be the order of reaction with respect of

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Exp.	$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	Initial rate $(m o l L^{- 1} s^{- 1})$
$1.$	$2.5 \times 10^{- 4}$	$3 \times 10^{- 5}$	$5 \times 10^{- 4}$
$2.$	$5 \times 10^{- 4}$	$6 \times 10^{- 5}$	$4 \times 10^{- 3}$
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$E x p$	$[X] (m o l L^{- 1})$	$[Y] (m o l L^{- 1})$	$I n i t i a l r a t e (m o l L^{- 1} s - 1)$
1.	$0.1$	$0.1$	$2 \times 10^{- 2}$
2.	$A$	$0.2$	$4 \times 10^{- 2}$
3.	$0.4$	$0.4$	$B$
4.	$C$	$0.2$	$2 \times 10^{- 2}$

Find the values of A, B and C in the following table for the reaction : X+Y⟶Z The reaction is first order with respect to X and zero order with respect to YExp[X](molL−1)[Y](molL−1)Initial rate(molL−1s−1)1.0.10.12×10−22.A0.24×10−23.0.40.4B4.C0.22×10−2

The correct option is A A=0.2 molL−1,B=8×10−2 molL−1s−1,C=0.1 molL−1

The correct option is A $A = 0.2 m o l L^{- 1}, B = 8 \times 10^{- 2} m o l L^{- 1} s^{- 1}, C = 0.1 m o l L^{- 1}$