Which of the following rate laws has an overall order of $0.5$ for reaction involving substances $x$, $y$ and $z$
Which of the following rate laws has an overall order of $0.5$ for reaction involving substances $x$, $y$ and $z$
- [AIIMS 1983]
- A
Rate $ = K({C_x})\,({C_y})\,({C_z})$
- B
Rate $ = K{({C_x})^{0.5}}\,{({C_y})^{0.5}}\,{({C_z})^{0.5}}$
- C
Rate $ = K{({C_x})^{1.5}}\,{({C_y})^{ - 1}}{({C_z})^0}$
- D
Rate $ = K({C_x})\,{({C_z})^n}/{({C_y})^2}$
Similar Questions
The reaction ${N_2}{O_5}$ (in $CCl_4$ solution) $ \to 2N{O_2}$ (solution) $ + \frac{1}{2}{O_2}(g)$ is of first order in ${N_2}{O_5}$ with rate constant $6.2 \times {10^{ - 1}}{s^{ - 1}}.$ What is the value of rate of reaction when $[{N_2}{O_5}] = 1.25\,mole\,{l^{ - 1}}$
The reaction ${N_2}{O_5}$ (in $CCl_4$ solution) $ \to 2N{O_2}$ (solution) $ + \frac{1}{2}{O_2}(g)$ is of first order in ${N_2}{O_5}$ with rate constant $6.2 \times {10^{ - 1}}{s^{ - 1}}.$ What is the value of rate of reaction when $[{N_2}{O_5}] = 1.25\,mole\,{l^{ - 1}}$
State a condition under which a bimolecular reaction is kinetically first order reaction.
State a condition under which a bimolecular reaction is kinetically first order reaction.
For $n^{th}$ order reaction where $(n < 1)$
For $n^{th}$ order reaction where $(n < 1)$
In a reaction between $A$ and $B$, the initial rate of reaction $\left(r_{0}\right)$ was measured for different initial concentrations of $A$ and $B$ as given below:
$A/mol\,\,{L^{ - 1}}$
$0.20$
$0.20$
$0.40$
$B/mol\,\,{L^{ - 1}}$
$0.30$
$0.10$
$0.05$
${r_0}/mol\,\,{L^{ - 1}}\,\,{s^{ - 1}}$
$5.07 \times 10^{-5}$
$5.07 \times 10^{-5}$
$1.43 \times 10^{-4}$
What is the order of the reaction with respect to $A$ and $B$?
In a reaction between $A$ and $B$, the initial rate of reaction $\left(r_{0}\right)$ was measured for different initial concentrations of $A$ and $B$ as given below:
| $A/mol\,\,{L^{ - 1}}$ | $0.20$ | $0.20$ | $0.40$ |
| $B/mol\,\,{L^{ - 1}}$ | $0.30$ | $0.10$ | $0.05$ |
| ${r_0}/mol\,\,{L^{ - 1}}\,\,{s^{ - 1}}$ | $5.07 \times 10^{-5}$ | $5.07 \times 10^{-5}$ | $1.43 \times 10^{-4}$ |
What is the order of the reaction with respect to $A$ and $B$?
For the first order decompsition reaction of $N_2O_5$, it is found that -
$(a)$ $2N_2O_5\rightarrow\,\,4NO_2(g)+O_2(g)-\frac{d[N_2O_5]}{dt}=k[N_2O_5]$
$(a)$ $N_2O_5\rightarrow\,\,2NO_2(g)+1/2\,\,O_2(g)-\frac{d[N_2O_5]}{dt}=k'[N_2O_5]$
which of the following is true ?
For the first order decompsition reaction of $N_2O_5$, it is found that -
$(a)$ $2N_2O_5\rightarrow\,\,4NO_2(g)+O_2(g)-\frac{d[N_2O_5]}{dt}=k[N_2O_5]$
$(a)$ $N_2O_5\rightarrow\,\,2NO_2(g)+1/2\,\,O_2(g)-\frac{d[N_2O_5]}{dt}=k'[N_2O_5]$
which of the following is true ?