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.

$C{H}_{3}COOH<mspace\; width="1em"></mspace>\stackrel{k_1}{\to }<mspace\; width="1em"></mspace>C{H}_4+<mspace\; width="1em"></mspace>C{O}_2$

$C{H}_{3}COOH<mspace\; width="1em"></mspace>\stackrel{k_2}{\to }<mspace\; width="1em"></mspace>C{H}_{2}CO<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>H_{2}O$

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

1. $\frac{50<mspace\; width="1em"></mspace>k_1}{\left(k_1+k_2\right)}$                                            

2. $\frac{100<mspace\; width="1em"></mspace>k_1}{\left(k_1+k_2\right)}$

3. $\frac{200<mspace\; width="1em"></mspace>k_1}{\left(k_1+k_2\right)}$                                           

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:

The kinetic data for the reaction: 2A + B₂ → 2AB are as given below

The order of reaction with respect to A and B₂ is, respectively:

For the irreversible unimolecular type reaction A $\stackrel{k}{\to }$products in a batch reactor, 80% reactant A($C_{A0}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1<mspace\; width="1em"></mspace>mole/lit.)$is converted in a 480 second run and conversion is 90% after 18 minute. The order of this reaction is-

(A) 1                                                       

(B) 2

(C) 1/2                                                   

(D) 3/2

The rate constant, the activation energy, and the Arrhenius parameter of a chemical reaction at 25°C are 3.0×10^-4 s^-1, 104.4 kJ mol^-1 and 6.0×10¹⁴s^-1 respectively.
The value of the rate constant as T → ∞ will be:

1. 2.0 × 10¹⁸ s^-1                                                  

2. 6.0 × 10¹⁴ s^-1

3. $\infty$                                                                   

4. 3.6 × 10³⁰ s^-1

The gas phase decomposition 2N₂O₅ → 4NO₂ + O₂ follows the first order rate law, K = 7.5 × 10^-3 sec^-1. The initial pressure of N₂O₅${\mathrm{<mspace\; width="1em"></mspace>}}_{}$is 0.1 atm. The time of decomposition of N₂O₅ so that the total pressure becomes 0.15 atm will be -

If in the fermentation of sugar in an enzymatic solution that is 0.12 M, the concentration of the sugar is reduced to 0.06 M in 10 h and to 0.03 M in 20 h, the order of the reaction will be:

1. 1                                                   

2. 2

3. 3                                                   

4. 0

In a first-order reaction A $\to$ products, the concentration of the reactant decreases to 6.25 % of its initial value in 80 minutes. The value of the rate constant, if the initial concentration is 0.2 mole/litre, will be:

1. $2.17$ $\times$ ${10}^{-2}$ $mi{n}^{-1}$

2. $3.46$ $\times$ ${10}^{-2}$ $mi{n}^{-1}$

3. $3.46$ $\times$ ${10}^{-3}mi{n}^{-1}$

4. $2.16$ $\times$ ${10}^{-3}$ $mi{n}^{-1}$