NEET Arrhenius Equation Practice Questions With Solutions

NEET Chemistry Arrhenius Equation Practice Questions

Question 1.

$C(s) + 2 H_2(g) \rightarrow CH_4(g); \Delta H = -74.8~kJ mol^{-1}$
Which of the following diagrams gives an accurate representation of the above reaction?
[R→reactants; P→products]

A

B

C

D

Question 2.

The rate of a reaction quadruples when temperature changes from 27°C to 57°C. Calculate the energy of activation.
Given R = 8.314 J K^–1 mol^–1, log 4 = 0.6021

1.	380.4 kJ/mol	2.	3.80 kJ/mol
3.	3804 kJ/mol	4.	38.04 kJ/mol

A380.4 kJ/mol

B3.80 kJ/mol

C3804 kJ/mol

D38.04 kJ/mol

Question 3.

Activation energy of any chemical reaction can be calculated if one knows the value of:

AProbability of collision.

BOrientation of reactant molecules during collision.

CRate constant at two different temperatures.

DRate constant at standard temperature.

Question 4.

Effective collisions are known to possess:

A: Energy greater than threshold energy.
B: Breaking of old bond in reactant.
C: Formation of new bond in product.
D: High activation energy.
E: Proper orientation.

Choose the correct answer from the options given below:

AA, B, C, D only

BA, B, C, E only

CA, C, D, E only

DB, C, D, E only

Question 5.

Rate constants of a reaction at 500 K and 700 K are 0.04 $s^{-1}$ and 0.14 $s^{-1}$, respectively; then, activation energy of the reaction is: (Given : log 3.5 = 0.5441, R = 8.31 J $K^{-1} $$\mathrm {mol}^{-1}$)

A182310 J

B18500 J

C18219 J

D18030 J

Question 6.

Which of the following plot represents the variation of $ln ~k$ versus $\frac 1{T}$ according to the Arrhenius equation?

A

B

C

D

Question 7.

The plot of ln k vs ${1 \over T}$ for the following reaction
$2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) $ gives a straight line with the slope of the line equal to $-1.0 \times 10^4 K $.
The activation energy for the reaction in J mol^–1 is:
(Given R = 8.3 J K^–¹ mol^–¹)

A$4.0 \times 10^2 $

B$4.0 \times 10^{-2} $

C$8.3 \times 10^{-4} $

D$8.3 \times 10^4 $

Question 8.

For a reaction A

\to

B, enthalpy of reaction is

- 4.2

kJ {mol}^{- 1}

and enthalpy of activation is

9.6

kJ {mol}^{- 1}

. The correct potential energy profile for the reaction is:

A

B

C

D

Question 9.

The slope of Arrhenius Plot (ln k v/s

\frac{1}{T}

) of the first-order reaction is

- 5 \times 10^{3}

K

. The value of E_a of the reaction is: [Given R = 8.314 JK^–1 mol^–1]

A166 kJ mol^–1

B–83 kJ mol^–1

C41.5 kJ mol^–1

D83.0 kJ mol^–1

Question 10.

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

AHeat of reaction

BThreshold energy

CCollision frequency

DActivation energy

Question 1.

What does Z_AB represent in the collision theory of chemical reactions?

AThe fraction of molecules with energies greater than E_a

BThe collision frequency of reactants, A and B

CSteric factor

DThe fraction of molecules with energies equal to E_a

Question 2.

For a reaction, activation energy $E_{a} = 0$ and the rate constant at 200 K is 1.6 $\times$ $10^{6} s^{- 1}$ . The rate constant at 400K will be [Given that gas constant, R=8.314 J $K^{- 1}$ $m o l^{- 1}$ ]

A3.2 × 10⁴ s^-1

B1.6 × 10⁶s^-1

C1.6 × 10³ s^-1

D3.2 × 10⁶ s^-1

Question 3.

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20^oC to 35^oC? (R = 8.314 J mol^–1 K^–1)

1.	269 kJ mol^–1	2.	34.7 kJ mol^–1
3.	15.1 kJ mol^–1	4.	342 kJ mol^–1

A269 kJ mol^–1

B34.7 kJ mol^–1

C15.1 kJ mol^–1

D342 kJ mol^–1

Question 4.

A reaction having equal energies of activation for forward and reverse reaction has:

AΔG = 0

BΔH = 0

CΔH = ΔG = ΔS = 0

DΔS = 0

Question 5.

For an endothermic reaction, the energy of activation is E_a, and the enthalpy of reaction is ΔH (both of these in kJ/mol). The minimum value of E_a will be:

ALess than

∆

H

BEqual to

∆

H

CMore than

∆

H

DEqual to zero

Question 6.

The rate constants k₁ and k₂ for two different reactions are 10¹⁶. e^-2000/T and 10¹⁵. e^-1000/T, respectively. The temperature at which k₁= k₂ is:

A

1000

K

B

\frac{2000}{2.303}

K

C

2000

K

D

\frac{1000}{2.303}

K

Question 7.

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

AIs negative of E_a

BIs always less than E_a

CCan be less than or more than E_a

DIs always double of E_a

Question 8.

The temperature dependence of the rate constant (k) of a chemical reaction is written in terms of the Arrhenius equation,
k = A.e^–E*/RT. The activation energy (E*) of the reaction can be calculated by plotting:

A

k

vs

T

B

k

vs

\frac{1}{\log}

T

C

\log

k

vs

\frac{1}{T}

D

\log

k

vs

\frac{1}{log T}

Question 9.

When a biochemical reaction is carried out in a laboratory outside the human body in the absence of an enzyme, then the rate of reaction obtained is $10^{- 6}$ times. The activation energy of a reaction in the presence of an enzyme is:

A

\frac{6}{R T}

BP is required.

CDifferent from

E_{a}

obtained in the laboratory.

DData is insufficient.

NEET Arrhenius Equation Practice Questions With Solutions

NEET Chemistry Arrhenius Equation Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

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