Order of a Reaction

For the reaction $2{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$, $\mathrm{r}=\mathrm{k}\left[{\mathrm{H}}_2{\mathrm{O}}_2\right]$. The reaction is of :

For the reaction ${\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}+{\mathrm{H}}_2\mathrm{O}\stackrel{ {\mathrm{H}}^{+} }{\to }{\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6+{\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6$, write the order of reaction.

What do you mean by molecularity and order of a reaction? Explain why their values are different in the reaction: ${\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5+{\mathrm{H}}_2\mathrm{O}\stackrel{ {\mathrm{H}}^{+} }{\to }{\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}$

Rate of reaction is the change in concentration of any one of the reactants or any one of the products in unit time. 

$2\mathrm{HI}\stackrel{ }{\to }{\mathrm{H}}_2+{\mathrm{I}}_2$

 The rate expression for the above reaction is $\mathrm{rate}=\mathrm{k} {\left[\mathrm{HI}\right]}^2$. Are the order and molecularity of the above reaction same? Give reason.

Rate of reaction is the change in concentration of any one of the reactants or any one of the products in unit time. 

$2\mathrm{HI}\stackrel{ }{\to }{\mathrm{H}}_2+{\mathrm{I}}_2$

 If the rate expression for the above reaction is $\mathrm{rate}=\mathrm{k} {\left[\mathrm{HI}\right]}^2$, what is the order of the reaction?

What is order of reaction? Write units of the rate constant $\mathrm{k}$ for zero order, first order and second order reaction.

Define the following:

Order of a reaction.

How is half-life period related to initial concentration for a second order reaction?
 

In the reaction $\mathrm{aA}+\mathrm{bB}\stackrel{ }{\to }\mathrm{Products}$, if concentration of $\mathrm{A}$ is doubled (keeping $\mathrm{B}$ constant) the initial rate becomes four times and if $\mathrm{B}$ is doubled (keeping $\mathrm{A}$ constant), the rate becomes double. What is the rate law equation and order of a reaction?

Define order of a reaction and molecularity of reaction. Derive a general expression for specific rate constant of first order reaction.

Give one example for a reaction where order and molecularity are equal.

Define the term 'order of reaction' for chemical reactions. 

Give an example for a reaction having fractional order.

The initial rate of reaction $\mathrm{A}+5 \mathrm{B}+6\mathrm{C}⟶3 \mathrm{L}+3\mathrm{M}$ has been determined by measuring the rate of disappearance of A under the following conditions:

$$\begin{gathered} \mathrm{Expt}. \mathrm{No}. [\mathrm{A}{]}_0/\mathrm{M} [\mathrm{B}{]}_0/\mathrm{M} [\mathrm{C}{]}_0/\mathrm{M} \mathrm{Initial} \mathrm{rate}/\mathrm{M}\min { }^{-1} \\ 1 0.02 0.02 0.02 2.08\times {10}^{-3} \\ 2 0.01 0.02 0.02 1.04\times {10}^{-3} \\ 3 0.02 0.04 0.02 4.16\times {10}^{-3} \\ 4 0.02 0.02 0.04 8.23\times {10}^{-3} \end{gathered}$$

Determine the order of reaction with respect to each reactant and overall order of the reaction. What is the rate constant? Calculate the initial rate of change in concentration of $\mathrm{B}$ and $\mathrm{L}$.

For the thermal decomposition of acetaldehyde, ${\mathrm{CH}}_3\mathrm{CHO}\left(\mathrm{g}\right)⟶{\mathrm{CH}}_4\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)$, the following rate data were obtained:

$$\begin{gathered} \mathrm{Experiment} \mathrm{Initial} \mathrm{pressure} \left(\mathrm{torr}\right) \mathrm{Initial} \mathrm{rate} \mathrm{of} \mathrm{increase} \mathrm{in} \mathrm{total} \mathrm{pressure} \left(\mathrm{torr}\right) \\ 1 300 0.61\left({\mathrm{r}}_1\right) \\ 2 600 0.27\left({\mathrm{r}}_2\right) \end{gathered}$$

Predict the order of reaction.

For the reaction $2{ \mathrm{N}}_2{\mathrm{O}}_5\left(\mathrm{g}\right)⟶4{\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$, the following results have been obtained:

$$\begin{gathered} \mathrm{S}.\mathrm{No}. \left[{\mathrm{N}}_2{\mathrm{O}}_5\right] \mathrm{mol} {\mathrm{L}}^{-1} \mathrm{Rate} \mathrm{of} \mathrm{disappearance} \mathrm{of} {\mathrm{N}}_2{\mathrm{O}}_5, \mathrm{mol} {\mathrm{L}}^{-1} {\min }^{-1} \\ 1 1.13\times {10}^{-2} 34\times {10}^{-5} \\ 2 0.84\times {10}^{-2} 25\times {10}^{-5} \\ 3 0.62\times {10}^{-2} 18\times {10}^{-5} \end{gathered}$$

Calculate the order of reaction.

The possible mechanism for the reaction: $2{\mathrm{H}}_2+2\mathrm{NO}⟶{\mathrm{N}}_2+2{\mathrm{H}}_2\mathrm{O}$ is

(i) $2\mathrm{NO}\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_2$ (ii) ${\mathrm{N}}_2{\mathrm{O}}_2+{\mathrm{H}}_2\to {\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\mathrm{O}$ (slow) (iii) ${\mathrm{N}}_2\mathrm{O}+{\mathrm{H}}_2\to {\mathrm{N}}_2+{\mathrm{H}}_2\mathrm{O}$ (fast)

What is the order of the reaction?

Define order of reaction.

The rate constant of a reaction is $3\times {10}^2 {\mathrm{h}}^{-1}$. What is the order of reaction?

For the reaction $2\mathrm{X}⟶{\mathrm{X}}_2$, the rate of reaction becomes $27$ times when the concentration of $\mathrm{X}$ is increased three times. What is the order of the reaction?