$A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$ but it is independent of the concentration of $B$, then
$A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$ but it is independent of the concentration of $B$, then
- A
The order of the reaction $2$ and molecularity $1$
- B
Molecularity of the reaction is $2$ but order is $1$
- C
Order is $ 2$ and molecularity is $2$
- D
Order of the reaction is $2$ but molecularity is $0$
Similar Questions
Write unit of rate constant of following reaction :
$1.$ fourth order
$2.$ third order
Write unit of rate constant of following reaction :
$1.$ fourth order
$2.$ third order
Which of these does not influence the rate of reaction
Which of these does not influence the rate of reaction
For the following reaction scheme (homogeneous), the rate constant has units
$A+B\xrightarrow{K}C$:
For the following reaction scheme (homogeneous), the rate constant has units
$A+B\xrightarrow{K}C$:
The mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is
$(i)\,\,N{O_2}\,\xrightarrow{{slow}}\,NO + O$
$(ii)\,\,{F_2} + O + NO\,\xrightarrow{{fast}}\,N{O_2}F + F$
$(iii)\,\,F + N{O_2}\,\xrightarrow{{fast}}\,N{O_2}F$
Select the correct one
The mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is
$(i)\,\,N{O_2}\,\xrightarrow{{slow}}\,NO + O$
$(ii)\,\,{F_2} + O + NO\,\xrightarrow{{fast}}\,N{O_2}F + F$
$(iii)\,\,F + N{O_2}\,\xrightarrow{{fast}}\,N{O_2}F$
Select the correct one
The experimental data for decomposition of $N _{2} O _{5}$
$\left[2 N _{2} O _{5} \rightarrow 4 NO _{2}+ O _{2}\right]$
in gas phase at $318 \,K$ are given below:
$t/s$
$0$
$400$
$800$
$1200$
$1600$
$2000$
$2400$
$2800$
$3200$
${10^2} \times \left[ {{N_2}{O_5}} \right]/mol\,\,{L^{ - 1}}$
$1.63$
$1.36$
$1.14$
$0.93$
$0.78$
$0.64$
$0.53$
$0.43$
$0.35$
$(i)$ Plot $\left[ N _{2} O _{5}\right]$ against $t$
$(ii)$ Find the half-life period for the reaction.
$(iii)$ Draw a graph between $\log \left[ N _{2} O _{5}\right]$ and $t$
$(iv)$ What is the rate law $?$
$(v)$ Calculate the rate constant.
$(vi)$ Calculate the half-life period from $k$ and compare it with $(ii)$.
The experimental data for decomposition of $N _{2} O _{5}$
$\left[2 N _{2} O _{5} \rightarrow 4 NO _{2}+ O _{2}\right]$
in gas phase at $318 \,K$ are given below:
| $t/s$ | $0$ | $400$ | $800$ | $1200$ | $1600$ | $2000$ | $2400$ | $2800$ | $3200$ |
| ${10^2} \times \left[ {{N_2}{O_5}} \right]/mol\,\,{L^{ - 1}}$ | $1.63$ | $1.36$ | $1.14$ | $0.93$ | $0.78$ | $0.64$ | $0.53$ | $0.43$ | $0.35$ |
$(i)$ Plot $\left[ N _{2} O _{5}\right]$ against $t$
$(ii)$ Find the half-life period for the reaction.
$(iii)$ Draw a graph between $\log \left[ N _{2} O _{5}\right]$ and $t$
$(iv)$ What is the rate law $?$
$(v)$ Calculate the rate constant.
$(vi)$ Calculate the half-life period from $k$ and compare it with $(ii)$.