Arrhenius Equation

Q.

The energy of activation of a first order reaction is $187.06kJmo{l}^{-1}$ at 750 K and the value of pre-exponential factor A is $1.97\times {10}^{12}{s}^{-1}$. Calculate the half life. $(e^{-30}=9.35\times {10}^{-14})$

1. 8.76s

2. 3.76s

3. 9.76s

4. 5.76s

Q.

The activation energy for a reaction at the temperature TK was found to be 2.303 $RTJmo{l}^{-1}$. The ratio of the rate constant to Arrhenius factor is ___

1. $2\times {10}^{-2}$

2. $2\times {10}^{-3}$

3. ${10}^{-2}$

4. ${10}^{-1}$

Q.

Does Arrhenius constant change with temperature?

Q.

Milk turns sour at ${40}^{\circ }$C three times as faster as $0^{\circ }$C. Hence, $E_a$ in the process of turning of milk sour is

1. $\frac{2.303\times 2\times 313\times 273}{40}log\left(1/3\right)cal$

2. $\frac{2.303\times 2\times 40}{273\times 313}log3cal$

3. None of these

4. $\frac{2.303\times 2\times 313\times 273}{40}log3$

Q. $Z{n}^{2+}+2e^{-}\to Zn$. The process happening in this reaction is:

1. reduction
2. None of the above
3. both
4. oxidation

Q.

For a first order reaction A ⟶ P, the temperature (T) dependent rate constant (k) was found to follow the equation log k = -2000(1/T) + 6.0. The pre-exponential factor A and the activation energy $E_a,$ respectively, are

(IIT-JEE, 2009)

1. $6.0s^{-1}and16.6kJmo{l}^{-1}$

2. $1.0\times {10}^6{s}^{-1}and16.6kJmo{l}^{-1}$

3. $1.0\times {10}^6{s}^{-1}and38.3kJmo{l}^{-1}$

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

Q.

What is the average rate of change for a function with the equation $2x+3y+6=0$?

Q. A decrease in Gibbs energy is a measure of maximum work done by the system.

Q.

The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

$(R=8.314J{K}^{-1}mo{l}^{-1}andlog2=0.301)$

(IIT-JEE-2013)

1. $48.6kJmo{l}^{-1}$

2. $58.5kJmo{l}^{-1}$

3. $60.5kJmo{l}^{-1}$

4. $53.6kJmo{l}^{-1}$