Definition Rate Constant Rate Law

For the reaction,

Which of the following is an incorrect expression for the rate of reaction?

1.		2.
3.		4.

Consider the reaction
N₂(g) + 3H₂(g) → 2NH₃(g)
The equality relationship between and is :

1. $\frac{d\left[N{H}_3\right]}{dt}=-\frac{1}{3}\frac{d\left[H_2\right]}{dt}$

2. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{2}{3}\frac{d\left[H_2\right]}{dt}$

3. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{3}{2}\frac{d\left[H_2\right]}{dt}$

4. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{d\left[H_2\right]}{dt}$

The bromination of acetone occurring in an acid solution is represented by the equation.
CH₃COCH₃(aq)+ Br₂(aq) →
CH₃COCH₂Br(aq) + H⁺(aq) + Br^-(aq)

The kinetic energy data were obtained for given reaction concentrations.
Initial concentrations, M
$\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$ $\left[{\mathrm{H}}^{+}\right]$

0.30 0.05 0.05

0.30 0.10 0.05

0.30 0.10 0.10

0.40 0.05 0.20
Initial rate, the disappearance of Br₂, Ms^-1
5.7 $\backslash times$ 10^-5

5.7 $\backslash times$ 10^-5

1.2 $\backslash times$ 10^-4

3.1 $\backslash times$ 10^-4
Based on the above data, the rate of the equation is:

1. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{H}}^{+}\right]$

2. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[\mathrm{CH}={\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$

3. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$ ${\left[{\mathrm{H}}^{+}\right]}^2$

4. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$ $\left[{\mathrm{H}}^{+}\right]$

Calculate the specific rate constant of the reaction if the half-life period of a first-order reaction is 1386 s?

1. $5.0\backslash times{10}^{-3}{s}^{-1}$

2. $0.5\backslash times{10}^{-2}{s}^{-1}$

3. $0.5\backslash times{10}^{-3}{s}^{-1}$

4. $5.0\backslash times{10}^{-2}{s}^{-1}$

For the reaction, A + B → products, it is observed that-
(1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
(2) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is given by:

1. $rate=k$ $\left[A{]}^2\right[B]$

2. $rate=k$ $\left[A\right][B{]}^2$

3. $rate=k$ $\left[A{]}^2\right[B{]}^2$

4. $rate=k$ $\left[A\right]\left[B\right]$

For the reaction, if, , the value of would be:
1.
2.
3.
4.

In the reaction,
${\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right)+5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+6{\mathrm{H}}^{+}\to$ 3Br₂(l)+3H₂O(l)
The rate of appearance of bromine (Br₂) is related to the rate of disappearance of bromide ions:

1. $\frac{d\left[B{r}_2\right]}{dt}=-\frac{3}{5}\frac{d\left[B{r}^{-}\right]}{dt}$

2. $\frac{d\left[B{r}_2\right]}{dt}=-\frac{5}{3}\frac{d\left[Br\right]}{dt}$

3. $\frac{d\left[B{r}_2\right]}{dt}=\frac{5}{3}\frac{d\left[B{r}^{-}\right]}{dt}$

4. $\frac{d\left[B{r}_2\right]}{dt}=\frac{3}{5}\frac{d\left[B{r}^{-}\right]}{dt}$

During the kinetic study of the reaction, 2A + B C + D, following results were obtained:

Run	[A)/ mol L-1	[B)/ mol L-1	Initial rate of formation of D/mol L-1
I	0.1	0.1	${\mathrm{}}^{}$
II	0.3	0.2	${\mathrm{}}^{}$
III	0.3	0.4	${\mathrm{}}^{}$
IV	0.4	0.1	${\mathrm{}}^{}$

Based on the above data which one of the following is correct?

1. rate= k[A]²[B]

2. rate= k[A][B]

3. rate= k[A]²[B]²

4. rate= k[A][B]²

Which of the following statements about the order of reaction is incorrect?

1.	Order is not influenced by the stoichiometric coefficient of the reactants.
2.	Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction.
3.	The order of reaction is always a whole number.
4.	Order can be determined by experiments only.

In a reaction, A + B → Product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8, when the concentrations of both the reactants (A and B) are doubled. The rate law for the reaction can be written as:

1. Rate = k[A][B]²

2. Rate = k[A]²[B]²

3. Rate = k[A][B]

4. Rate = k[A]²[B]

The correct statement among the following is:

1.	the rate of a first-order reaction does not depend on reactant concentration; the rate of a second-order reaction does depend on reactant concentrations.
2.	the half-life of a first-order reaction does not depend on [A]o; the half-life of a second-order reaction does depend on [A]0
3.	a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed.
4.	the rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations

For the chemical reaction ${\mathrm{N}}_2\left(\mathrm{(g)}\right)+3{\mathrm{H}}_2\left(\mathrm{(g}\right)$ )$\rightleftharpoons$ $2{\mathrm{NH}}_3\left(\mathrm{(g)}\right)$ the correct option is:

1.		2.
3.		4.