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(B) The graph shows $[R]$ vs $t$. Reaction $1$,$2$,and $3$ represent decreasing concentrations with time.For zero-order reactions,$[R] = [R]_{0} - kt$

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The rate constant of reaction $3$ is larger than the rate constant of reaction $2$ if the order of reaction is the same for both.

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(B) The graph shows $[R]$ vs $t$. Reaction $1$,$2$,and $3$ represent decreasing concentrations with time.For zero-order reactions,$[R] = [R]_{0} - kt$,which is a straight line. As the order increases,the curves become more convex.Reaction $1$ is a straight line (zero-order),Reaction $2$ is first-order,and Reaction $3$ is second-order.The unit of the rate constant for zero-order is $mol 	ext{ L}^{-1} 	ext{ s}^{-1}$. Thus,option $C$ is incorrect.For a fixed initial concentration,the rate constant order is $k_{3} > k_{2} > k_{1}$ to maintain the decay profiles,as reaction $3$ decays faster than $2$. Therefore,option $B$ is correct.

Consider the given graph showing the variation of reactant concentration with time. Three different reactions were started with identical initial concentration of reactants. Which of the following statements is correct?

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