For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.

The order of the reaction will be:

1. 3                                                      

2. 2

3. 1                                                      

4. 0

The rate constant of a first-order reaction is typically determined from a plot of:

1. Concentration of reactant vs time t

2. Log (concentration of reactant) vs time t

3. \(\frac{1}{\text { concentration of reactant }} \text { vs time } t\)
4. Concentration of reactant vs log time t

The relationship between temperature and the variance in reaction rate is:

1.		2.
3.		4.

The plot of log k versus $\frac{1}{T}$ is linear with a slope of

(1) $\frac{E_a}{R}$                                                    

(2) $\frac{-E_a}{R}$

(3) $\frac{E_a}{2.303R}$                                             

(4) $\frac{-E_a}{2.303R}$

If a reaction A + B $\to$ C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy of 70 kJ/mol, the activation energy for the reverse reaction will be:

1. 30 kJ/mol                                       

2. 40kJ/mol

3. 70 kJ/mol                                       

4. 100 kJ/mol

A first-order reaction takes 40 min for 30 % decomposition. The t_1/2 for this reaction will be:

For a certain reaction involving a single reactant, it is found that $C_0\sqrt{T}$ is constant where $C_0$is the initial concentration of the reactant and T is the half-life. What is the order of the reaction ?

(1) 1                                              

(2) Zero

(3) 2                                              

(4) 3

The high temperature ($\approx$ 1200K) decomposition of $C{H}_{3}COOH$(g) occurs as follows as per simultaneous 1st order reactions.

$C{H}_{3}COOH \stackrel{k_1}{\to } C{H}_4+ C{O}_2$

$C{H}_{3}COOH \stackrel{k_2}{\to } C{H}_{2}CO + H_{2}O$

What would be the % of $C{H}_4$by mole in the product mixture (excluding$C{H}_{3}COOH$)?

1. $\frac{50 k_1}{\left(k_1+k_2\right)}$                                            

2. $\frac{100 k_1}{\left(k_1+k_2\right)}$

3. $\frac{200 k_1}{\left(k_1+k_2\right)}$                                           

4. it depends on the time

The reaction , A(g) + 2B(g) C(g) + D(g) is an elementary process. In an experiment, the initial partial pressure of A and B are $P_A$= 0.60 and $P_B$= 0.80 atm. When $P_C$= 0.2atm the rate of reaction relative to the initial rate is

(1) 1/48                                                               

(2) 1/24

(3) 9/16                                                              

(4) 1/6

The half-life period for a first-order reaction is 20 minutes. The time required to change the concentration of the reactants from 0.08 M to 0.01 M will be: