For a general reaction $A \to B$, plot of concentration of $A$ vs time is given in figure. Answer the following question on the basis of this graph.
$(i)$ What is the order of the reaction ?
$(ii)$ What is the slope of the curve ?
$(iii)$ What are the units of rate constant ?
For a general reaction $A \to B$, plot of concentration of $A$ vs time is given in figure. Answer the following question on the basis of this graph.
$(i)$ What is the order of the reaction ?
$(ii)$ What is the slope of the curve ?
$(iii)$ What are the units of rate constant ?
$(i)$ Zero order reaction.
For zero order reaction
$[\mathrm{R}]=-k(t)+[\mathrm{R}]_{0}$
$\uparrow$
$y=m$ $\begin{array}{lll}\uparrow & \uparrow & \uparrow \\ x & + & c\end{array}$
So, the graph is of straight line.
$(ii)$ Slope $=-k$
$(iii)$ Unit of zero order reaction is $\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}$.
Similar Questions
For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.
$t$ $(sec)$
$P(m m \text { of } H g)$
$0$
$35.0$
$360$
$54.0$
$720$
$63.0$
Calculate the rate constant.
For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.
| $t$ $(sec)$ | $P(m m \text { of } H g)$ |
| $0$ | $35.0$ |
| $360$ | $54.0$ |
| $720$ | $63.0$ |
Calculate the rate constant.
The rate constant k, for the reaction ${N_2}{O_5}(g) \to $ $2N{O_2}(g) + \frac{1}{2}{0_2}(g)$ is $2.3 \times {10^{ - 2}}\,{s^{ - 1}}$. Which equation given below describes the change of $[{N_2}{O_5}]$ with time? ${[{N_2}{O_5}]_0}$ and ${[{N_2}{O_5}]_t}$ correspond to concentration of ${N_2}{O_5}$ initially and at time $t$.
The rate constant k, for the reaction ${N_2}{O_5}(g) \to $ $2N{O_2}(g) + \frac{1}{2}{0_2}(g)$ is $2.3 \times {10^{ - 2}}\,{s^{ - 1}}$. Which equation given below describes the change of $[{N_2}{O_5}]$ with time? ${[{N_2}{O_5}]_0}$ and ${[{N_2}{O_5}]_t}$ correspond to concentration of ${N_2}{O_5}$ initially and at time $t$.
- [AIIMS 2004]
For a chemical reaction, $A + 2B \to C + D$, the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\, times$, then rate of reaction also increases $2\, times$. The order of this reaction is
For a chemical reaction, $A + 2B \to C + D$, the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\, times$, then rate of reaction also increases $2\, times$. The order of this reaction is
The reaction $2 A + B _{2} \rightarrow 2 AB$ is an elementary reaction.
For a certain quantity of reactants, if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).
The reaction $2 A + B _{2} \rightarrow 2 AB$ is an elementary reaction.
For a certain quantity of reactants, if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).
- [JEE MAIN 2021]
Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
take place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$
The order of the reaction is
Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
take place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$
The order of the reaction is