Half-lives of a first order and a zero order | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) For a first order reaction,the rate is given by $Rate_1 = k_1 [A]_0$,where $k_1 = \frac{0.693}{t_{1/2}}$. Thus,$Rate_1 = \frac{0.693 [A]_0}{t_{1/2

Vedclass · Accepted Answer

$2 	imes 0.693$

Vedclass · Answer

(B) For a first order reaction,the rate is given by $Rate_1 = k_1 [A]_0$,where $k_1 = \frac{0.693}{t_{1/2}}$. Thus,$Rate_1 = \frac{0.693 [A]_0}{t_{1/2}}$.For a zero order reaction,the rate is given by $Rate_0 = k_0$,where $k_0 = \frac{[A]_0}{2 t_{1/2}}$.Given that the half-lives $(t_{1/2})$ are the same for both reactions,the ratio of the initial rates is:$\frac{Rate_1}{Rate_0} = \frac{\frac{0.693 [A]_0}{t_{1/2}}}{\frac{[A]_0}{2 t_{1/2}}} = 0.693 	imes 2 = 1.386$.

Half-lives of a first order and a zero order reaction are same. Then the ratio of the initial rates of first order reaction to that of the zero order reaction is

Similar Questions

For a chemical reaction, half-life period $(t_{1/2})$ is $10 \ minutes$. How much reactant will be left after $20 \ minutes$ if one starts with $100 \ moles$ of reactant and the order of the reaction is $(i)$ zero, $(ii)$ one, and $(iii)$ two?

Select the incorrect statement.

For a first order reaction,which of the following statements is correct?

The decomposition of $N_2O_5$ follows first-order kinetics: $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$. Its half-life is $2.4 \ hours$. If $10.8 \ g$ of $N_2O_5$ is taken initially,how many liters of $O_2$ will be obtained at $STP$ after $9.6 \ hours$?

The given graph is a representation of kinetics of a reaction. The $y$ and $x$ axes for zero and first order reactions,respectively are

Vedclass Test Series

Exam Paper Generator

Online Exam Module