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The effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation) Mock Test for JEE

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Part of Chemical Kinetics in JEE Main Chemistry.

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Q1ChemistryUnit 8: Chemical Kinetics

H_{2}

reacts much faster with

C l_{2}

then

D_{2}

because:

Q2ChemistryUnit 8: Chemical Kinetics

Which of the following rules states that with the increase of every

10^{\circ} \mathrm{C}

temperature the rate of metabolic activity gets doubled?

Q3ChemistryUnit 8: Chemical Kinetics

Which of the following statements is not correct about physisorption?

Q4ChemistryUnit 8: Chemical Kinetics

Which one of the following statements is false? This question has multiple correct options

Q5ChemistryUnit 8: Chemical Kinetics

Rate of disappearance of the reactant

\boldsymbol{A}

at two different temperature is given by

\boldsymbol{A} \rightleftharpoons \boldsymbol{B}

\frac{-\boldsymbol{d}[\boldsymbol{A}]}{\boldsymbol{d t}}=\left(\boldsymbol{2} \times \mathbf{1 0}^{-2} \boldsymbol{S}^{-1}\right)[\boldsymbol{A}]-\boldsymbol{4} \times

\mathbf{1 0}^{-3} \boldsymbol{S}^{-\mathbf{1}}[\boldsymbol{B}], \boldsymbol{T}=\mathbf{3 0 0} \boldsymbol{K}

\frac{-\boldsymbol{d}[\boldsymbol{A}]}{\boldsymbol{d t}}=\left(\boldsymbol{4} \times \mathbf{1 0}^{-2} \boldsymbol{S}^{-1}\right)[\boldsymbol{A}]-\mathbf{1 6} \times

\mathbf{1 0}^{-\mathbf{4}}[\boldsymbol{B}], \boldsymbol{T}=\mathbf{4 0 0} \boldsymbol{K}

Calculate heat of reaction in the given temperature range, when equilibrium is

\operatorname{set}

up.

Q6ChemistryUnit 8: Chemical Kinetics

N_{2}(g)+3 H_{2}(g) \rightleftharpoons 2 N H_{3}(g)+22

kcal. The activation energy for the forward reaction 50 kcal. What is the activation energy for the backward reaction?

Q7ChemistryUnit 8: Chemical Kinetics

The rate constant for a reaction can be increased by

\underline{a}

the stability of the reactant or by

\underline{b}

the stability of the transition state. Select the correct choice for a and

b

Q8ChemistryUnit 8: Chemical Kinetics

Catalysts lower the activation energy of a reaction:

Q9ChemistryUnit 8: Chemical Kinetics

What are effective collisions? This question has multiple correct options

Q10ChemistryUnit 8: Chemical Kinetics

Graph between log k and 1/T [k is rate constant

\left(s^{-1}\right)

and

T

the temperature (K)

]

is a straight line with

0 X=5, \theta=

\tan ^{-1}(1 / 2.303) .

Hence

-E_{a}

will be :

Q11ChemistryUnit 8: Chemical Kinetics

In the Arrhenius equation

k=A e^{E / R T}

rate will be constant at:

Q12ChemistryUnit 8: Chemical Kinetics

Why do most chemical reaction rates increase rapidly as the temperature rises

Q13ChemistryUnit 8: Chemical Kinetics

A chemical reaction was carried out at

300 \mathrm{K}

and

280 \mathrm{K}

. The rate constants were found to be

K_{1}

and

K_{2}

300 \mathrm{K}

and

280 \mathrm{K}

respectively. Then which of the following is true?

Q14ChemistryUnit 8: Chemical Kinetics

A reaction takes place in three steps with an individual rate constant and activation energy, as given below. Rate constant Activation energy Step 1

\quad \boldsymbol{k}_{\mathbf{1}} \quad \boldsymbol{E}_{\boldsymbol{a}_{1}}=

180 k J / m o l

Step 2

\quad \boldsymbol{k}_{2} \quad \boldsymbol{E}_{\boldsymbol{a}_{2}}=

\mathbf{8 0 k J} /

mol Step 3

\quad k_{3} \quad \quad E_{a_{3}}=

\mathbf{5 0 k J / m o l}

And overall rate constant,

k=

\left(\frac{k_{1} k_{2}}{k_{3}}\right)^{2 / 3}

The overall activation energy of the reaction will be:

Q15ChemistryUnit 8: Chemical Kinetics

Assertion The pressure of a fixed amount of an ideal gas is proportional to its temperature Reason Frequency of collisions and their impact both increase in proportion to the square root of temperature

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