A. $\rightarrow$ (1) B. $\rightarrow$ (2) C. $\rightarrow$ (2) D. $\rightarrow$ (1)

For zero order reaction rate equation may be written as

$$[R]=-k t+\left[R_0\right]\quad\text{.... (i)}$$

Which denotes a straight line equation similar to $y=m x+c$

On transforming (i)

$$\begin{aligned} \frac{[R]-\left[R_0\right]}{t} & =-k \\ k & =\frac{\left[R_0\right]-[R]}{t} \end{aligned}$$

$$\begin{aligned} k & =\text { Rate } \\ \text { Rate } & =k \cdot[t]^0 \\ \text { Rate } & \propto[t]^0 \end{aligned}$$

For a first order reaction $\frac{d x}{d t} \propto[\text{concentration}]^{1}$

$\therefore$ Graph between rate and concentration may be drawn as

$$\begin{aligned} k & =\frac{2.303}{t} \log \frac{[R]_0}{[R]} \\ \frac{k t}{2.303} & =\log \left[\frac{R^{\circ}}{R}\right] \\ \frac{k t}{2.303} & =\log [R]_0-\log [R]\\ \log [R]&=\underset{\text { Slope }}{\left(\frac{-k}{2.303}\right)} t+\underset{\text { Intercept }}{\log [R]_0} \end{aligned}$$

A. $\rightarrow(3)$ B. $\rightarrow$ (1) C. $\rightarrow$ (4) D. $\rightarrow$ (6) E. $\rightarrow$ (2) F. $\rightarrow$ (5)

1. Catalyst alters the rate of reaction by lowering activation energy.

2. Molecularity can't be fraction or zero. If molecularity is zero, then reaction is not possible.

3. Second half-life of first order reaction is same as first because half-life time is temperature independent.

4. $e^{-E_Q / R T}$ refers to the fraction of molecules with kinetic energy equal to or greater than activation energy.

5. Energetically favourable reactions are sometimes slow due to improper orientation of molecule cause some ineffective collision of molecules.

6. Area under the Maxwell, Boltzmann curve is constant because total probability of molecule taking part in a chemical reaction is equal to one.

A. $\rightarrow(2)$ B. $\rightarrow$ (1) C. $\rightarrow$ (3)

1. Diamond can't be converted into graphite under ordinary condition.

2. Instantaneous rate of reaction completes at very short span of time.

3. Average rate of reaction occurs to a long duration of time.

$\mathrm{A.\rightarrow (2)}$ $\quad \mathrm{B} \rightarrow(1) \quad \mathrm{C} \rightarrow(4) \quad \mathrm{D} \rightarrow(3)$

1. Mathematical expression for rate of reaction is known as rate law.

2. Rate of reaction for zero order reaction is equal to rate constant

$$\begin{aligned} & r=k[A]^0 \\ \therefore\quad& r=k \end{aligned}$$

3. Unit of rate of reaction is same as that of rate of reaction.

4. Order of complex reaction is determined by rate of a reaction, which is slowest.