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(B) To determine the order of the reaction,we check the rate of change of concentration with respect to time.For a zero-order reaction,the rate is con

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(B) To determine the order of the reaction,we check the rate of change of concentration with respect to time.For a zero-order reaction,the rate is constant: $Rate = -\frac{d[R]}{dt} = k$.Let's calculate the rate for different intervals:Interval $1$: $t = 0$ to $0.05 \ min$,$\Delta [R] = 1.0 - 0.76 = 0.24 \ M$,$\Delta t = 0.05 \ min$. Rate $= \frac{0.24}{0.05} = 4.8 \ M \ min^{-1}$.Interval $2$: $t = 0.05$ to $0.12 \ min$,$\Delta [R] = 0.76 - 0.40 = 0.36 \ M$,$\Delta t = 0.07 \ min$. Rate $= \frac{0.36}{0.07} \approx 5.14 \ M \ min^{-1}$.Interval $3$: $t = 0.12$ to $0.18 \ min$,$\Delta [R] = 0.40 - 0.10 = 0.30 \ M$,$\Delta t = 0.06 \ min$. Rate $= \frac{0.30}{0.06} = 5.0 \ M \ min^{-1}$.Since the rate of reaction is approximately constant $(4.8, 5.14, 5.0)$,the reaction follows zero-order kinetics.

$[R] \ (M)$	$1.0$	$0.76$	$0.40$	$0.10$
$t \ (min)$	$0.0$	$0.05$	$0.12$	$0.18$

For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained:

$[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$

$t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$

The order of the reaction is:

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For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained: $[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$ $t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$ The order of the reaction is: