Order of Reaction

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

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

Q. For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope. The order of the reaction is-

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

Q. For the reaction 2A + 3B $\to$products, A is in excess and on changing the concentration of B from 0.1 M to 0.4 M, rate becomes doubled. Thus, rate law is

1. $\frac{dx}{dt}=k\left[A{]}^2\right[B{]}^2$
2. $\frac{dx}{dt}=k\left[A\right]\left[B\right]$
3. $\frac{dx}{dt}=k\left[A\right]0[B{]}^2$
4. $\frac{dx}{dt}=k[B{]}^{1/2}$

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

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

Q. Which one of the following is a second order reaction?

1. $H_2+C{l}_2\to 2HCl$
2. $H_2+B{r}_2\to 2HBr$
3. $N{H}_{4}N{O}_3\to N_2+3H_{2}O$
4. $C{H}_{3}COOC{H}_3+NaOH\to C{H}_{3}COONa+C{H}_{3}OH$

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

Q. Rate constant for a $n^{th}$ order reaction has the dimensions
(Where M is concentration unit)

1. $tim{e}^{-1}{M}^{(1-n)}$
2. $tim{e}^{1-n}{M}^{-1}$
3. $tim{e}^1{M}^{(1-n)}$
4. $tim{e}^{-1}{M}^{1+n}$

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. 2
4. 1.5