Rate of Reaction

Q. The rate of a chemical reaction doubles for every $10{}^{\circ }C$ rise of temperature. If the temperature is raised by $50{}^{\circ }C$, the rate of the reaction increase by about

Q.

The rate of a chemical reaction doubles for every $10°\mathrm{C}$ rise in temperature. If the temperature is raised by $50°\mathrm{C}$, the rate of the reaction increases by about.

Q. If α is the degree of dissociation of Na2SO4. The vant Hoff factor used for the calculation of molecular mass is Options: Correct 1 + 2α 1 – α 1 + α 1 – 2α

Q.

For the reaction, $N_2{O}_5\left(g\right)\to N{O}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)$ The value of rate of disappearance of $N_2{O}_5$ is given as $6.25\times {10}^{-3}mol{L}^{-1}{s}^{-1}.$ The rate of formation of $N{O}_2$ and $O_2$ is given respectively as:

1. $6.25\times {10}^{-3}mol{L}^{-1}{s}^{-1}and6.25\times {10}^{-3}mol{L}^{-1}{s}^{-1}$

2. $1.25\times {10}^{-2}mol{L}^{-1}{s}^{-1}and3.125\times {10}^{-3}mol{L}^{-1}{s}^{-1}$

3. $6.25\times {10}^{-3}mol{L}^{-1}{s}^{-1}and3.125\times {10}^{-3}mol{L}^{-1}{s}^{-1}$

4. $1.25\times {10}^{-}2mol{L}^{-1}{s}^{-1}and6.25\times {10}^{-3}mol{L}^{-1}{s}^{-1}$

Q.

The rate constant, activation energy and Arrhenius parameter of a chemical reaction at 25^oC are 3.0 x 10^-4 s^-1, 104.4 kJ mol^-1 and 6.0 x 10¹⁴ s^-1 respectively. The value of the rate constant at infinite temperature is is

1. Infinity

2. 6.0 x 10¹⁴ s^-1

3. 2 x 10¹⁸ s^-1

4. 6.0 x 10³⁰ s^-1

Q.

Explain the difference between instantaneous rate of reaction and average rate of a reaction.

Q.

A reaction is first order in A and second order in B:

Write the differential rate equation.

How is the rate affected on increasing the concentration of B three times?

How is the rate affected when the concentrations of both A and B are doubled?

Q.

The following data were obtained during the first order thermal decomposition of SO₂Cl₂ at a constant volume.

Experiment	Time/s−1	Total pressure/atm
1	0	0.5
2	100	0.6

Calculate the rate of the reaction when total pressure is 0.65 atm.

Q.

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.
$\begin{array}{cccc}A/mol{L}^{-1}& 0.20& 0.20& 0.40\\ B/mol{L}^{-1}& 0.30& 0.10& 0.05\\ x_0/mol{L}^{-1}{s}^{-1}& 5.07\times {10}^{-5}& 5.07\times {10}^{-5}& 1.43\times {10}^{-4}\end{array}$
What is the order to the reaction with respect to A and B?

Q. Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide:
$2NO\left(g\right)+O_2\left(g\right)\to 2N{O}_2\left(g\right)$
If the mechanism of reaction is;
$NO+O_2\stackrel{k}{\rightleftharpoons }N{O}_3\left(fast\right)$
$N{O}_3+NO\stackrel{k_1}{⟶}N{O}_2+N{O}_2\left(slow\right)$
The rate law is:

1. Rate=$k^{\prime }\left[NO\right]\left[O_2\right]$
2. Rate=$k^{\prime }\left[NO\right][O_2{]}^2$
3. Rate=$k^{\prime }\left[NO{]}^2\right[O_2]$
4. Rate=$k^{\prime }\left[NO{]}^3\right[O_2]$

Q. In a chemical reaction, the rate constant for the backward reaction is $7.5\times {10}^{-4}$ and the equilibrium constant is $1.5$ the rate constant for forward reaction is:

1. $5\times {10}^{-4}$
2. $1.125\times {10}^{-3}$
3. $9\times {10}^{-4}$
4. $2\times {10}^{-3}$

Q.

Which of the following statements is correct ?
(a) The rate of reaction decreases with passage of time as the concentration of reactants decreases
(b) The rate of reaction is same at any time during the reaction
(c) The rate of a reaction is independent of temperature change
(d) The rate of a reaction decreases with increase in concentration of reactant (s)

Q. The value of Kc = 4.24 at 800 Kfor the reaction CO(g) + H2O (g) gives rise to CO2(g) + H2(g) Calculate equilibrium concentrations of CO2, H2, CO and H2O at 800 K , if only CO and H2O are present initially at concentration of 0.10 M each ?

Q.

The initial concentration of cane sugar is presence of an acid was reduced from 0.20 to 0.1M in 5hours and to 0.05M in 10hours value of K ?

Ans .0.1368/hour pls put it on paper

Q. The following mechanism has been proposed for the reaction of NO with $B{r}_2$ to form NOBr
$N{O}_{\left(g\right)}+B{r}_{2_{\left(g\right)}}\rightleftharpoons NOB{r}_{2\left(g\right)}NOB{r}_{2\left(g\right)}+N{O}_{\left(g\right)}\to 2NOB{r}_{\left(g\right)}$
If the second step is the rate determining step, the order of the reaction with respect to $N{O}_{\left(g\right)}$ is

1. 1
2. 0
3. 2
4. 3

Q.

The number of collisions per second per unit volume of the reaction mixture is known as:

1. Boltzmann factor

2. Activated complex

3. Collision frequency

4. Activation energy

Q.

Define promotors and inhibitors.

Q. From the following data, the decomposition of $H_2{O}_2$ in aqueous solution follows first order kinetics. Then calculate its rate constant (k) value.

Time (in minutes)	0	10	20
Volume (V) in $mL$	22	13	7.5

where V is the volume of potassium permanganate required to react with undecomposed hydrogen peroxide solution.

Take
$log\frac{22}{13}=0.23log\frac{22}{7.5}=0.46$

1. $k=0.053mi{n}^{-1}$
2. $k=0.102mi{n}^{-1}$
3. $k=0.204mi{n}^{-1}$
4. $k=0.40mi{n}^{-1}$

Q. In a reaction, the concentration of a reactant (A) changes from $0.200mol{L}^{-1}$ to $0.150mol{L}^{-1}$ in 10 minutes. What is the average rate of reaction during this interval ?

1. $0.005\text{mol}{L}^{-1}{\text{min}}^{-1}$
2. $0.05\text{mol}{L}^{-1}{\text{min}}^{-1}$
3. $0.01\text{mol}{L}^{-1}{\text{min}}^{-1}$
4. $0.5\text{mol}{L}^{-1}{\text{min}}^{-1}$

Q. Assertion : Hydrolysis of ester in acidic medium follows first order kinetics Reason: Hydrolysis ofester is independent of the concentration of acid used

Q. Find the rate law that corresponds to the data shown for the following reaction?

Experiment	$\left[A_0\right]=M$	$\left[B_0\right]=M$	Initial rate
1	0.012	0.035	0.10
2	0.024	0.070	0.80
3	0.024	0.035	0.10
4	0.012	0.070	0.080

1. $\text{Rate}=\left[A{]}^2\right[B{]}^2$
2. $\text{Rate}=k[B{]}^4$
3. $\text{Rate}=k\left[A\right][B{]}^3$
4. $\text{Rate}=k\left[A{]}^0\right[B{]}^3$

Q.

Why does the rate of any reaction generally decreases during the course of the reaction?

Q. Ammonia and oxygen reacts at higher temperatures as
$4N{H}_3\left(g\right)+5O_2\left(g\right)\to 4NO\left(g\right)+6H_{2}O\left(g\right)$
In an experiment, the concentration of $NO$ increases by $2.16\times {10}^{–2}{\text{mol litre}}^{–1}$ in $3$ seconds.

Which of the following is correct?

1. Rate of the reaction is $7.2\times {10}^{-3}mol{L}^{-1}{s}^{-1}$
2. Rate of disappearance of ammonia is $7.2\times {10}^{-3}mol{L}^{-1}{s}^{-1}$
   
3. Rate of formation of water is $4.32\times {10}^{-2}mol{L}^{-1}{s}^{-1}$
4. Rate of disappearance of oxygen is $3.6\times {10}^{-2}mol{L}^{-1}{s}^{-1}$

Q.

What does the Iron Cycle involve?

Q.

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 L−1	B/ mol L−1	Initial rate/mol L−1 min−1
I	0.1	0.1	2.0 × 10−2
II	--	0.2	4.0 × 10−2
III	0.4	0.4	--
IV	--	0.2	2.0 × 10−2

Q. The temperature coefficient for the saponification of ethyl acetate by $NaOH$ is 1.75 when the temperatures rises from ${25}^{o}C$ to ${35}^{o}C$. Calculate activation energy for the saponification of ethyl acetate.
Take,
${\log }_{10}\left(1.75\right)=0.243$

1. $E_a=42.7kJmo{l}^{-1}$
2. $E_a=14.0kJmo{l}^{-1}$
3. $E_a=64.4kJmo{l}^{-1}$
4. $E_a=2.6kJmo{l}^{-1}$

Q. The rate constant for the reaction A B is $2\times {10}^{-4}lt.mo{l}^{-1}mi{n}^{-1}.$The concentration of A at which rate of the reaction is \( (1/20) \times 10^{-5} \) M/sec. is

1. $\left(1/20\right)\sqrt{5/3}$
2. 0.25 M
3. 0.5 M
4. None of these

Q.

Compounds 'A' and 'B' react according to the following chemical equation.

$A\left(g\right)+2B\left(g\right)⟶2C\left(g\right)$

Concentration of either 'A' or 'B' were changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

$\begin{array}{cccc}Experiment& InitialConcentrationof\left[A\right]/moI{L}^{-1}& Initialcooncentrationof\left[B\right]/moI{L}^{-1}& Initialcooncentrationof\left[C\right]/moI{L}^{-1}{s}^{-1}\\ 1.& 0.30& 0.30& 0.10\\ 2.& 0.30& 0.60& 0.40\\ 3.& 0.60& 0.30& 0.20\end{array}$
$\left(a\right)Rate=k\left[A{]}^2\right[B\left]\right(b)Rate=k[A\left]\right[B{]}^2\left(c\right)Rate=k\left[A\right]\left[B\right]\left(d\right)Rate=k\left[A{]}^2\right[B{]}^0$

Q. The hydrolysis of an ester was carried out separately with 0.05M HCl and 0.05 M H2SO4. Which of the following will be true (A) K(HCI) > K(H2SO4) (B) K(HCI) < K(H2SO4) (C) K(HCI) = K(H2SO4)(D) K(HCI) = 2 K(H2SO4) here K is rate constant

Q. Write structures of different isomeric alkyl groups corresponding to the molecular formula $C_5{H}_{11}$. Write IUPAC name of alcohols obtained by attachment of $-OH$ groups at different carbons of the chain.