Order of Reaction

Q.

The rate equation for the reaction 2A + B $\to$ C is found to be: rate = k[A][B]. The correct statement in relation of this reaction is that the

1. Rate of formation of C is twice the rate of disappearance of A
2. Unit of k is $s^{-1}$
3. $t_{\frac{1}{2}}$ is a constant
4. Value of k is independent of the initial concentration of A and B

Q. Find the $E^0$ value for the reaction,
$I{n}^{2+}\left(aq\right)+C{u}^{2+}\left(aq\right)\rightleftharpoons I{n}^{3+}\left(aq\right)+C{u}^{+}\left(aq\right)$ at $298K$.
Given:
$E_{C{u}^{2+}\left(aq\right)/C{u}^{+}\left(aq\right)}^0=0.15V{E}_{I{n}^{2+}\left(aq\right)/I{n}^{+}\left(aq\right)}^0=-0.4V$
$E_{I{n}^{3+}\left(aq\right)/I{n}^{+}\left(aq\right)}^0=-0.42V$

Q. The kinetic energy of $N$ molecules of $O_2$ is $x$ joule at $-{123}^{\circ }\text{C}$. Another sample of $O_2$ at ${27}^{\circ }\text{C}$ has a kinetic energy of $2x$. The latter sample contains ____ molecules of $O_2$:

1. $N$
2. $\frac{N}{2}$
3. $2N$
4. $3N$

Q. For reaction: A + B $\to$ Products, the rate if the reaction at various concentration are given below:
$\begin{array}{cccc}Expt.No.& \left(A\right)& \left(B\right)& Rate\\ 1& 0.2& 0.2& 2\\ 2& 0.2& 0.4& 4\\ 3& 0.6& 0.4& 36\end{array}$

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

Q. Karthik is carrying out a reaction with chemicals A and B according to the reaction, $(3A\to B)$. He wants to find the order of the reaction by changing concentration of A and observing the rate of the reaction. The first observation he made was by increasing the concentration of A 4 times after which, the rate of reaction doubled. Can you guess the order of reaction using Karthik’s experimental observation?

1. 1
2. 0.5
3. 1.5
4. 2

Q. For the reaction A + B $\to$ C, it is found that doubling the concentration of A increases the rate by 4 times and doubling the concentration of B doubles the reaction rate. What is the overall order of the reaction?

1. 4
2. $\frac{3}{2}$
3. 3
4. 1

Q. If $H{g}_{2}C{l}_2$ is 80% ionised in the aqueous solution what will be the van't Hoff factor of $H{g}_{2}C{l}_2$ in the solution?

1. 1.6
2. 2.6
3. 3.6
4. 4.6

Q. For reaction: A + B $\to$ Products, the rate if the reaction at various concentration are given below:
$\begin{array}{cccc}Expt.No.& \left(A\right)& \left(B\right)& Rate\\ 1& 0.2& 0.2& 2\\ 2& 0.2& 0.4& 4\\ 3& 0.6& 0.4& 36\end{array}$

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

Q.

Which one of the following statement(s) is incorrect about order of reaction?

1. Order of reaction is determined experimentally

2. Order of reaction is equal to sum of the power of concentration terms in differential rate law

3. It is not affected with stoichiometric coefficient of the reactants

4. Order cannot be fractional

Q. At ${518}^{\circ }C$ the rate of decomposition of a sample of gaseous acetaldehyde initially at a pressure of 363 Torr, was 1.00 Torr $s^{-1}$ when 5% had reacted and 0.5 Torr $s^{-1}$ when 33% had reacted. The order of the reaction is:

1. \N
2. 2
3. 3
4. 1

Q. Arun setup a reaction in a lab $[2A\to B]$. All the information he has is that it is a second order reaction. Now he wants to increase the rate of the reaction 16 times. He knows that by increasing the concentration, the rate increases, but he doesn’t know what the final concentration has to be. Can you help him find it?

1. Increase the concentration of A by 2 times.
2. Increase the concentration of A by 3 times.
3. Increase the concentration of A by 8 times.
4. Increase the concentration of A by 4 times.

Q. Rate constant of a reaction is $175litr{e}^{2}mo{l}^{-2}se{c}^{-1}$. What is the order of reaction?

Q. The conversion of molecules A to B follows second order kinetics. Doubling the concentration of A will increase the rate of formation of B by a factor of

1. $2$
2. $4$
3. $\frac{1}{2}$
4. $\frac{1}{4}$

Q. Identify the order of the reaction from the following rate constants respectively
a. $k=7.06\times {10}^{-3}{\text{mol}}^{-1}{\text{L s}}^{-1}$
b. $k=5.60\times {10}^{-5}{\text{s}}^{-1}$
c. $k=1.25\times {10}^{-2}{\text{mol L}}^{-1}{\text{s}}^{-1}$
d. $k=1.25\times {10}^{-2}{\text{mol}}^{-2}{\text{L}}^2{\text{s}}^{-1}$

1. $0,1,2,3$
2. $2,1,0,3$
3. $3,1,0,2$
4. $3,0,1,2$

Q. The rate law expression for four reactions are give below. In which case, the percentage increase in the rate of reaction would be maximum when the concentration of A is doubled?

1. $r=k\left[A\right]$
2. $r=k[A{]}^{\frac{3}{2}}$
   
   
3. $r=k[A{]}^{\circ }$
4. $r=k[A{]}^2$

Q. The following results have been obtained during the kinetic study of the reaction
$A+B⟶C+D$
$\begin{array}{cccc}\text{Experiment}& \text{[A]}& \text{[B]}& \text{Initial rate of}\\ & & & \text{formation of}\\ & & & \left(Mse{c}^{-1}\right)\\ \text{I}& 0.1& 0.1& 6.0\times {10}^{-3}\\ \text{II}& 0.3& 0.2& 7.2\times {10}^{-2}\\ \text{III}& 0.3& 0.4& 2.88\times {10}^{-1}\\ \text{IV}& 0.4& 0.1& 2.40\times {10}^{-2}\end{array}$
Determine the rate law of the above reaction.

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

Q. For the reaction A + B $\to$ C, it is found that doubling the concentration of A increases the rate by 4 times and doubling the concentration of B doubles the reaction rate. What is the overall order of the reaction?

1. 4
2. $\frac{3}{2}$
3. 3
4. 1

Q. For a reaction X $\to$ Y, the rate of the reaction has been found to be third order with respect to X. What happens when the concentration of X is doubled.

1. rate become double
2. rate becomes three times
3. rate become six times
4. rate becomes eight times

Q.

The equation that describes mathematically the dependence of the rate of reaction on the concentration terms of reactants is _____or______.

Q. Arun setup a reaction in a lab $[2A\to B]$. All the information he has is that it is a second order reaction. Now he wants to increase the rate of the reaction 16 times. He knows that by increasing the concentration, the rate increases, but he doesn’t know what the final concentration has to be. Can you help him find it?

1. Increase the concentration of A by 2 times.
2. Increase the concentration of A by 3 times.
3. Increase the concentration of A by 8 times.
4. Increase the concentration of A by 4 times.

Q. Karthik is carrying out a reaction with chemicals A and B according to the reaction, $(3A\to B)$. He wants to find the order of the reaction by changing concentration of A and observing the rate of the reaction. The first observation he made was by increasing the concentration of A 4 times after which, the rate of reaction doubled. Can you guess the order of reaction using Karthik’s experimental observation?

1. 1
2. 0.5
3. 1.5
4. 2

Q. $2X\left(g\right)+3Y\left(g\right)+Z\left(g\right)\to P\left(g\right)+Q\left(g\right)$
The order of the given reaction is $\frac{3}{4}$ and the experimental rate law of the given reaction is $K\left[X{]}^{\frac{1}{2}}\right[Y{]}^{\frac{3}{4}}[Z{]}^a$. Find the order of reaction with respect to Z.

1. $0$
2. $\frac{1}{2}$
3. $1$
4. $\frac{-1}{2}$