Which graph represents a zero order reaction | vedclass

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(D) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.$Rate = -\frac{d[A]}{dt} = \frac{d[B]}{dt} = k[

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(D) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.$Rate = -\frac{d[A]}{dt} = \frac{d[B]}{dt} = k[A]^0 = k$.$1$. The concentration of product $[B]$ increases linearly with time $t$ $([B] = kt + [B]_0)$.$2$. The rate of formation of product,$\frac{d[B]}{dt}$,is constant and independent of time $t$.$3$. The half-life period $t_{1/2}$ is directly proportional to the initial concentration $[A]_0$ $(t_{1/2} = \frac{[A]_0}{2k})$.$4$. The time for $3/4$ completion,$t_{3/4}$,is also directly proportional to the initial concentration $[A]_0$ $(t_{3/4} = \frac{3[A]_0}{4k})$.Looking at the provided options:- Option $A$ shows $[B]$ vs $t$ as a constant line,which is incorrect.- Option $B$ shows $\frac{d[B]}{dt}$ vs $t$ as a linear increase,which is incorrect.- Option $C$ shows $t_{1/2}$ vs $[A]_0$ as a constant line,which is incorrect.- Option $D$ shows $t_{3/4}$ vs $[A]_0$ as a linear graph passing through the origin,which is correct for a zero order reaction.

$Time \ (s)$	$Rate \ (mol \ L^{-1} s^{-1})$
$0$	$1.60 \times 10^{-2}$
$10$	$1.60 \times 10^{-2}$
$20$	$1.60 \times 10^{-2}$
$30$	$1.60 \times 10^{-2}$

Which graph represents a zero order reaction $[A_{(g)} \to B_{(g)}]$?

Similar Questions

Which of the following plots is correct for a zero-order reaction?

Consider the data given below for the hypothetical reaction $A \to X$:
$Time \ (s)$ $Rate \ (mol \ L^{-1} s^{-1})$
$0$ $1.60 \times 10^{-2}$
$10$ $1.60 \times 10^{-2}$
$20$ $1.60 \times 10^{-2}$
$30$ $1.60 \times 10^{-2}$

From the above data,the order of the reaction is:

The reaction $A \to \text{Products}$ is a zero-order reaction. If the initial concentration of $A$ is $2 \ M$,then at time $t = 1/K$ (where $K$ is the rate constant),the concentration of $A$ will be ......... $M$.

Mention True $(T)$ and False $(F)$ statements for the following regarding a zero-order reaction $R \rightarrow P$:
$1. \ t_{1/2} \propto [R]_0$
$2. \ t_{1/2} \propto k$

If the rate of the reaction is equal to the rate constant,the order of the reaction is

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