Order of Reaction

Q. For a reaction:
$3A\to$ products
It is found that the rate of reaction doubles when the concentration of $A$ is increased by four times. What is the order of the reaction?

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

Q. For a reaction $pA+qB\to \text{product}$, the rate law expression is $r=k\left[A{]}^l\right[B{]}^m$, then:

1. $(p+l)<(l+m)$
2. $(p+q)>(l+m)$
3. $(p+q)$ may or may not be equal to $(l+m)$
4. $(p+q)=(l+m)$

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. If in the given reaction, 3I_2 + OH^- → IO_3^-+ 5I^- , 2 moles of iodine are taken, then the ratio of iodate and iodide ions formed in the alkaline medium is

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:
$E_{C{u}^{2+}\left(aq\right)/C{u}^{+}\left(aq\right)}^0=0.15V{E}_{I{n}^{2+}\left(aq\right)/I{n}^{+}\left(aq\right)}^0=-0.4V$
$E_{I{n}^{3+}\left(aq\right)/I{n}^{+}\left(aq\right)}^0=-0.42V$

1. $0.59V$
2. $0.97V$
3. $1.23V$
4. $0.23V$

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. Mechanism of a hypothetical reaction $X_2+Y_2\to 2XY$ is given below :
(i)$X_2\to X+X$ (fast)
(ii) $X+Y_2\rightleftharpoons XY+Y$ (slow)
(iii) $X+Y\to XY$ (fast)
The overall order of the reaction will be:

1. 1
2. 2
3. \N
4. 1.5

Q. The gaseous reaction: $A\left(g\right)+nB\left(g\right)\rightleftharpoons mC\left(g\right)$ is represented by following curves. What is the value of $n+m$?

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.

If I is the intensity of absorbed light and C is the concentration of AB for the photochemical process $AB+hV\to AB$,
then the rate of formation of AB is directly proportional to?

1. C

2. I

3. $I^2$

4. C.I

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. The gaseous reaction: $A\left(g\right)+nB\left(g\right)\rightleftharpoons mC\left(g\right)$ is represented by following curves. What is the value of $n+m$?

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. 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. What will be the $E^0$ value for the given half cell reaction?
$S{n}^{4+}\left(aq\right)+4e^{-}\to Sn\left(s\right)$
Given:
$E^0$ value for the half cell reaction,
$S{n}^{4+}\left(aq\right)+2e^{-}\to S{n}^{2+}\left(aq\right);E^0=0.15V$
$S{n}^{2+}\left(aq\right)+2e^{-}\to Sn\left(s\right);E^0=-0.14V$

1. $-0.001V$
2. $-0.005V$
3. $+0.001V$
4. $+0.005V$

Q.

what is oxidation number of oxygen in ozone?explain it.

Q. From the given table for reaction between A and B:
$\begin{array}{ccccc}& & & \text{Initial rate}& \text{Initial rate}\\ & \left[A\right]{\text{mol litre}}^{-1}& \left[B\right]{\text{mol litre}}^{-1}& \text{at 300 K}& \text{at 320 K}\\ & & & {\text{mol litre}}^{-1}{\text{s}}^{-1}& {\text{mol litre}}^{-1}{\text{s}}^{-1}\\ \text{(I)}& 2.5\times {10}^{-4}& 3.0\times {10}^{-5}& 5.0\times {10}^{-4}& 2.0\times {10}^{-3}\\ \text{(II)}& 5.0\times {10}^{-4}& 6.0\times {10}^{-5}& 4.0\times {10}^{-3}& -\\ \text{(III)}& 1.0\times {10}^{-3}& 6.0\times {10}^{-5}& 1.6\times {10}^{-2}& -\end{array}$

Rate constant at $300\text{K}$ is $x\times {10}^8{\text{mol}}^{-2}{\text{litre}}^2{\text{s}}^{-1}$. Find the value of $15x$.

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