For a first order reaction A → P , the temperature T dependent rate constant k was found to follow the equation logk =- 2000 1 T + 6 .0 . The pre-exponential factor A and the activation energy E a , respectively, are

1.0 × 10 6 s - 1 and 38.3 kJ mol - 1

1.0 × 10 6 s - 1 and 9.2 kJ mol - 1

1.0 × 10 6 s - 1 and 16.6 kJ mol - 1

EASY

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Which of the following statement(s) $i s / a r e$ true

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Important Questions on Chemical Kinetics

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

For the following reactions

A \overset{700 K}{\to} Product

A \overset{500 K}{\underset{catalyst}{\to}} Product

It was found that the

E_{a}

is decreased by

30 K J / m o l

in the presence of catalyst. If the rate remains unchanged, the activation energy for catalysed reaction is (Assume pre-exponential factor is same)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

Consider the given plots for a reaction obeying Arrhenius equation $(0 ° C < T < 300 ° C) :$ ( $K$ and $E_{a}$ are rate constant and activation energy, respectively )

(I)

Question Image

(II)

Question Image

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

For a first order reaction

A \to P,

the temperature

(T)

dependent rate constant

(k)

was found to follow the equation

logk =- (2000) \frac{1}{T} + 6 .0 .

The pre-exponential factor A and the activation energy

E_{a},

respectively, are

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

For an endothermic reaction, where

ΔH

represent the enthalpy of reaction in

kJ {mol}^{- 1}

, the minimum value for energy of activation (for forward reaction) will be

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

In collision theory of chemical reaction,

Z_{AB}

represents

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

What is activation energy of a reaction?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

Higher order

(> 3)

reactions are rare due to

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

The unit of activation energy is

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

The rate constants for a reaction at

400 K

and

500 K

are

2.60 \times 10^{- 5} s^{- 1}

and

2.60 \times 10^{- 3} s^{- 1}

,respectively. The activation energy of the reaction in

{kJmol}^{- 1}

is ______

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

The temperature coefficient of a reaction is

2

. When the temperature is increased from

30 ° C

90 ° C

, the rate of reaction is increased by

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

For a reversible reaction, $A ⇌ B$ , which one of the following statement is wrong from the given energy profile diagram?

Question Image

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

The rate of a reaction A doubles on increasing the temperature from

300 to 310 K

. By how much, the temperature of reaction B should be increased from

300 K

so that rate doubles if activation energy of the reaction B is twice to that of reaction A.

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

If the first order rate constants for the decomposition of ethyl iodide at

600 K

and

700 K

are

2.0 \times 10^{- 5} s^{- 1}

and

2.0 \times 10^{- 4} s^{- 1}

respectively, the activation energy for this reaction in

{kJmol}^{- 1}

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

Define activation energy.

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

The specific rate of a reaction quadruples when temperature changes from

30^{o} C

50^{o} C

. Calculate energy of activation of the reaction in

{kJmol}^{- 1}

(to the closest integer).
(

R = 8.314 J K^{- 1} {mol}^{- 1}

)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

Define activation energy.

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

An exothermic reaction

X \to Y

has an activation energy

30 kJ {mol}^{- 1}

. If energy change

ΔE

during the reaction is

- 20 kJ

, then the activation energy for the reverse reaction in

kJ

is (Integer answer)

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

298 K

temperature the activation energy for the reaction

x_{2} + y_{2} \to 2 xy + 20 kJ

15 kJ .

What will be the activation energy for the reaction

2 xy \to x_{2} + y_{2} ?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

An increase in the concentration of the reactants of a reaction leads to change in

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Collision Theory of Chemical Reaction

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 = {8.314 JK}^{-1} {mol}^{-1} and log 2 = 0.301)

Which of the following statement(s) is/are true

Important Questions on Chemical Kinetics

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Which of the following statement(s) $i s / a r e$ true