The reaction that occurs in a breath analyser, a device used to determine the alcohol level in a person's blood stream is
$2 \mathrm{~K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}+8 \mathrm{H}_{2} \mathrm{SO}_{4}+3 \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} \rightarrow 2 \mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}+$
$3 \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}+2 \mathrm{~K}_{2} \mathrm{SO}_{4}+11 \mathrm{H}_{2} \mathrm{O}$
If the rate of appearance of $\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ is $2.67 \,\mathrm{~mol}$ $\min ^{-1}$ at a particular time, the rate of disappearance of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ at the same time is ...... $\mathrm{mol}\, \mathrm{min}^{-1}$ (Nearest integer)
The reaction that occurs in a breath analyser, a device used to determine the alcohol level in a person's blood stream is
$2 \mathrm{~K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}+8 \mathrm{H}_{2} \mathrm{SO}_{4}+3 \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} \rightarrow 2 \mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}+$
$3 \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}+2 \mathrm{~K}_{2} \mathrm{SO}_{4}+11 \mathrm{H}_{2} \mathrm{O}$
If the rate of appearance of $\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ is $2.67 \,\mathrm{~mol}$ $\min ^{-1}$ at a particular time, the rate of disappearance of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ at the same time is ...... $\mathrm{mol}\, \mathrm{min}^{-1}$ (Nearest integer)
- [JEE MAIN 2021]
- A
$3$
- B
$2$
- C
$4$
- D
$1$
Similar Questions
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
- [NEET 2017]
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 instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56\times10^{-3}\,Ms^{-1}$, $2MnO_4^-+ 10I^-+ 16 H^+ \to 2 Mn^{2+} + 5I_2 + 8H_2O$ The rate of appearance $I_2$ is
The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56\times10^{-3}\,Ms^{-1}$, $2MnO_4^-+ 10I^-+ 16 H^+ \to 2 Mn^{2+} + 5I_2 + 8H_2O$ The rate of appearance $I_2$ is
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
Experiment
$[ A ] / mol\, ^{-1}$
$[ B ] / mol\, ^{-1}$
Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$
$I$
$0.1$
$0.1$
$2.0 \times 10^{-2}$
$II$
-
$0.2$
$4.0 \times 10^{-2}$
$III$
$0.4$
$0.4$
-
$IV$
-
$0.2$
$2.0 \times 10^{-2}$
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
| Experiment | $[ A ] / mol\, ^{-1}$ | $[ B ] / mol\, ^{-1}$ | Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | - | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | - |
| $IV$ | - | $0.2$ | $2.0 \times 10^{-2}$ |
If initial concentration is reduced to its $1/4^{th}$ in a zero order reaction, the time taken for half of the reaction to complete
If initial concentration is reduced to its $1/4^{th}$ in a zero order reaction, the time taken for half of the reaction to complete