In the Arrhenius plot of ln k vs \(\frac{1}{T}\) a linear plot is obtained with a slope of –2 × 10⁴ K. The energy of activation of the reaction (in kJ mole^-1) is (R value is 8.3J K^-1 mol^-1)

Solution

For a reaction, activation energy (E_a) = 0 and rate constant k = 3.2 × 10⁶s^-1 at 300 K. What is the value of the rate constant at 310 K

3.2 × 10^-12s^-1
3.2 × 10⁶s^-1
6.4 × 10¹²s^-1
6.4 × 10⁶s^-1

Solution

When E_a = 0 rate constant is independent of temperature.

The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by 10°C is

The value of threshold energy increases
Collision frequency increases
The fraction of the molecule having energy equal to threshold energy or more increases
Activation energy decreases

Solution

When the temperature is increased, energy in form of heat is supplied which increases the kinetic energy of the reacting molecules. this will increase the number of collisions and ultimately the rate of reaction will be enhanced.

Which one of the following reactions is a true first order reaction?

Alkaline hydrolysis of ethyl acetate
Acid catalyst hydrolysis of ethyl acetate
Decomposition of N₂O
Decomposition of gaseous ammonia on a hot platinum surface

Solution

The minimum energy a molecule should possess in order to enter into a fruitful collision is known as

reaction energy
collision energy
activation energy
threshold energy

Solution

The definition of threshold energy.

Rate of a reaction can be expressed by Arrhenius equation as:
k = Ae^-E_a/RT
In this equation, E_a represents

the total energy of the reacting molecules at a temperature, T
the fraction of molecules with energy greater than the activation energy of the reaction
the energy below which all the colliding molecules will react
the energy below which colliding molecules will not react

Solution

In Arrhenius equation k = Ae^-E_a/RT, E_a is the energy of activation, which is required by the colliding molecules to react resulting in the formation of products

The activation energy for a simple chemical reaction A ⟶ B is E_a in forward direction. The activation energy for reverse reaction

is always double of E_a
is negative of E_a
is always less than E_a
can be less than or more than E_a

Solution

For a first order reaction, the time taken to reduce the initial concentration by a factor of \(\frac{1}{4}\) is 20 minutes. The time required to reduce initial concentration by a factor of \(\frac{1}{16}\) is

20 min
10 min
80 min
40 min

Solution

Solution

The rate law for the reaction xA + yB ⟶ mP + nQ is Rate = k [A]^c[B]^d. What is the total order of the reaction?

(x + y)
(m + n)
(c + d)
x/y

Solution

Order is the sum of the powers to which the concentration terms are raised in the rate equation.

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