The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}}\, = \,\frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high
The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}}\, = \,\frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high
- A
$0$
- B
$3$
- C
$1$
- D
$2$
Similar Questions
For a chemical reaction $A \rightarrow B$, it was found that concentration of $B$ is increased by $0.2\, mol\,L^{-1}$ in $30\, \mathrm{~min}$. The average rate of the reaction is $......\times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~h}^{-1}$. (Nearest integer)
For a chemical reaction $A \rightarrow B$, it was found that concentration of $B$ is increased by $0.2\, mol\,L^{-1}$ in $30\, \mathrm{~min}$. The average rate of the reaction is $......\times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~h}^{-1}$. (Nearest integer)
- [JEE MAIN 2021]
The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of ....... The order of the reaction is
${N_2}$ in $cc$
$6.25$
$9.50$
$11.42$
$13.65$
$35.05$
Time (minutes)
$10$
$15$
$20$
$25$
Finally
The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of ....... The order of the reaction is
| ${N_2}$ in $cc$ | $6.25$ | $9.50$ | $11.42$ | $13.65$ | $35.05$ |
| Time (minutes) | $10$ | $15$ | $20$ | $25$ | Finally |
If order of a reaction is $x$ then unit of it's rate constant is
If order of a reaction is $x$ then unit of it's rate constant is
Why can’t molecularity of any reaction be equal to zero ?
Why can’t molecularity of any reaction be equal to zero ?
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$