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(A) The average rate of a reaction is defined as the change in concentration of a reactant or product divided by the time interval taken for the chang

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$\frac{|x-y|}{100}$

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(A) The average rate of a reaction is defined as the change in concentration of a reactant or product divided by the time interval taken for the change.For the reaction $A ightarrow B$,the average rate is given by:$	ext{Average Rate} = -\frac{\Delta[A]}{\Delta t}$Here,the change in concentration of $A$ is $\Delta[A] = [A]_{final} - [A]_{initial} = y - x$.The time interval is $\Delta t = 100 \ \min$.Therefore,the average rate is $-\frac{y - x}{100} = \frac{x - y}{100}$.Since rate is always positive,we take the magnitude: $\frac{|x - y|}{100} \ mol \ L^{-1} \ \min^{-1}$.

$t/s$	$0$	$50$	$100$	$150$	$200$	$300$	$400$	$700$	$800$
$[C_{4}H_{9}Cl]/mol\ L^{-1}$	$0.100$	$0.0905$	$0.0820$	$0.0741$	$0.0671$	$0.0549$	$0.0439$	$0.0210$	$0.017$

$A \rightarrow B$ is a first order reaction. The concentration of $A$ is decreased from $x \ mol \ L^{-1}$ to $y \ mol \ L^{-1}$ in $100 \ \min$. What is the average velocity of the reaction in $mol \ L^{-1} \ \min^{-1}$?

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