(B) The rate law for a reaction of order $x$ is given by: $Rate = K[Concentration]^{x}$.The unit of rate is $mol \, L^{-1} \, sec^{-1}$ and the unit o

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$mol^{1-x} \, L^{x-1} \, sec^{-1}$

(B) The rate law for a reaction of order $x$ is given by: $Rate = K[Concentration]^{x}$.The unit of rate is $mol \, L^{-1} \, sec^{-1}$ and the unit of concentration is $mol \, L^{-1}$.Substituting these units into the rate law: $mol \, L^{-1} \, sec^{-1} = K \times (mol \, L^{-1})^{x}$.Solving for $K$: $K = \frac{mol \, L^{-1} \, sec^{-1}}{(mol \, L^{-1})^{x}} = mol^{1-x} \, L^{x-1} \, sec^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

If the order of a reaction is $x$,then the unit of its rate constant is:

A
$mol^{x-1} \, L^{1-x} \, sec^{-1}$
B
$mol^{1-x} \, L^{x-1} \, sec^{-1}$
C
$mol^{1-x} \, L^{x-1} \, sec$
D
$mol^{x-1} \, L^{x-1} \, sec^{-1}$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

Which of the following is an example of a second-order reaction?

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For the reaction $2A + B \rightarrow C$,the rate law is given by: $\text{Rate} = k[A][B]$. Which of the following statements is correct regarding this reaction?

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........ of a reaction cannot be determined experimentally.

EasyTS EAMCET 2004

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$

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For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

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$N_2$ volume in $cc$ $(V_t)$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$ $(V_{\infty})$
Time $(t)$ in minutes	$10$	$15$	$20$	$25$	$\infty$

If the order of a reaction is $x$,then the unit of its rate constant is:

Similar Questions

Which of the following is an example of a second-order reaction?

For the reaction $2A + B \rightarrow C$,the rate law is given by: $\text{Rate} = k[A][B]$. Which of the following statements is correct regarding this reaction?

........ of a reaction cannot be determined experimentally.

The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:$N_2$ volume in $cc$ $(V_t)$$6.25$$9.50$$11.42$$13.65$$35.05$ $(V_{\infty})$Time $(t)$ in minutes$10$$15$$20$$25$$\infty$

For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$