Which one of the following statements is wron | vedclass

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Question

(NONE) The correct answer is not explicitly listed as a 'wrong' statement among the options provided,as all statements $A, B, C,$ and $D$ are scientif

Vedclass · Accepted Answer

Order of a reaction depends upon the mechanism of the reaction.

Vedclass · Answer

(NONE) The correct answer is not explicitly listed as a 'wrong' statement among the options provided,as all statements $A, B, C,$ and $D$ are scientifically correct.$1$. Molecularity is the number of reacting species taking part in an elementary reaction,which must be a whole number.$2$. Order is an experimental quantity,while molecularity is a theoretical concept; they are often different.$3$. Zero-order reactions are common (e.g.,photochemical reactions).$4$. Order is determined by the rate-determining step in a reaction mechanism.However,if the question implies identifying a false statement,all provided options are actually true in chemical kinetics.

$[A] \ (mol/L)$	$[B] \ (mol/L)$	Rate $(mol/L \cdot s)$
$0.05$	$0.05$	$1.2 \times 10^{-3}$
$0.10$	$0.05$	$2.4 \times 10^{-3}$
$0.05$	$0.10$	$1.2 \times 10^{-3}$

$Exp$	$[A]_0$	$[B]_0$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

Which one of the following statements is wrong?

Similar Questions

Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$

$0.05$ $0.05$ $1.2 \times 10^{-3}$

$0.10$ $0.05$ $2.4 \times 10^{-3}$

$0.05$ $0.10$ $1.2 \times 10^{-3}$

The rate of reaction $A + 2B \to 3C$ becomes $72$ times when the concentration of $A$ is tripled and the concentration of $B$ is doubled. The order of reaction with respect to $A$ and $B$ respectively is:

For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.

The following are the rate constants of two different reactions. Determine the overall order of reaction for each case:
$(a)$ $6.66 \times 10^{-3} \, s^{-1}$
$(b)$ $4.5 \times 10^{-2} \, mol^{-1} \, L \, s^{-1}$

The data for the reaction $A + B \to C$ is given below:

$Exp$ $[A]_0$ $[B]_0$ Initial Rate

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.035$ $0.80$

$3$ $0.012$ $0.070$ $0.10$

$4$ $0.024$ $0.070$ $0.80$

Determine the rate law for the reaction.

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