Activation Energy

Q.

What is the relation between rate constant and Activation energy?

Q. For a first order reaction, A $\to$ P, the temperature (T) dependent rate constant (k) was found to follow the equation:
$logk=\frac{2000}{T}+6.0$
the pre - exponential factor A and the activation energy $E_{\alpha }$. respectively, are:

1. $1.0\times {10}^6{s}^{-1}and16.6kJmo{l}^{-1}$
2. $1.0\times {10}^6{s}^{-1}and38.3kJmo{l}^{-1}$
3. $1.0\times {10}^6{s}^{-1}and9.2kJmo{l}^{-1}$
4. $6.0s^{-1}and16.6kJmo{l}^{-1}$

Q. Which of the following statements are true?
1. ​ LPG, matchstick, coal, and petrol are the examples of combustible substances. ​
2. Substances that have a higher ignition temperature than room temperature undergo spontaneous combustion.​
3. Burning of kerosene is an example of rapid combustion.​
4. Carbon monoxide is produced during complete combustion of coal.​ ​

1. 1 and 3 ​
2. 1, 2, and 3 ​
3. 2, 3, and 5 ​
4. 3 and 4 ​

Q.

The activation energies for the forward and reverse elementary reactions in the system $A\rightleftharpoons B$ are 10.303 and 8.000 k cal respectively at 500K. Assuming the pre-exponential factor to be the same for both the forward and reverse steps and R = 2 cal $K^{-1}mo{l}^{-1}$, calculate equilibrium constant of the reaction :

1. 10.0

2. 100

3. 0.1

4. 1.00