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CHXII04:CHEMICAL KINETICS

320239 The minimum energy required for a reaction to take place is called

1 Internal energy

2 Threshold energy

3 Activation energy

4 Free energy

CHXII04:CHEMICAL KINETICS

320240 Which among the following equation represents Arrhenius equation?

1

{k = A}_{e}^{E_{a} / R T}

2

k = A . e^{R T / E_{a}}

3

k = \frac{A}{e^{E_{a} / R T}}

4

k = \frac{A}{e^{R T / E_{a}}}

Explanation:

Variation of rate constant $k$ with temperature $T (K)$ is given by Arrhenius equation.
It is based on the two theories of reaction rates, i.e., collision theory and transition state theory.
$k = A e^{- E_{a} / R T} = \frac{A}{e^{E a / R T}} (1)$
where ' $A$ ' is called the frequency factor or the pre-exponential factor.
$E_{a}$ is activation energy $e^{- E_{a} / R T}$ is referred as Boltzmann factor. A, has same unit as the rate constant. Collectively $A$ and $E_{a}$ are called the Arrhenius parameters of the reaction.

CHXII04:CHEMICAL KINETICS

320241 A reactant (1) forms two products

$A \overset{k_{1}}{\to} B$ , Activation energy $E_{a_{1}}$

$A \overset{k_{2}}{\to} C$ , Activation energy $E_{a_{2}}$

If ${(E_{a})}_{2} = 2 {(E_{a})}_{1}$ then $k_{1} and k_{2}$ are related as

1

k_{2} = k_{1} e^{E_{a_{2}} /RT}

2

k_{1} = k_{2} e^{E_{a_{1}} /RT}

3

k_{1} = A k_{2} e^{E_{a_{1}} /RT}

4

k_{1} = 2 k_{2} e^{E_{a_{2}} /RT}

Explanation:

$A \overset{k_{1}}{⟶} B, A \overset{k_{2}}{⟶} C$
By Arrhenius equation,
$\begin{aligned} k_{1} = A^{'} e^{- E_{α_{l}} / R T} \\ ∴ E_{a_{2}} = 2 E_{a_{1}} \\ ∴ k_{2} = A^{'} e^{- E_{a_{1}} / R T} \\ \frac{k_{1}}{k_{2}} = \frac{A^{'} e^{- E_{q_{1}} / R T}}{A^{'} e^{- E_{α_{2}} / R T}} = e^{E_{q_{1}} / R T} \\ ∴ k_{1} = k_{2} e^{E_{q /} / R T} \end{aligned}$
and $k_{2} = A^{'} e^{- E_{q_{2}} / R T} [A^{'}$ is Arrhenius constant $]$

CHXII04:CHEMICAL KINETICS

320242 Which plots will give the value of activation energy?

1 k Vs T

2

1 / k V s T

3

l n k V s T

4

l n k V s 1 / T

Explanation:

According to Arrhenius equation,
$k = {Ae}^{- E_{a} / RT} \Rightarrow \ln k = \ln A - \frac{E_{a}}{RT}$
Rearrange the above equation in the form of
$\begin{aligned} y = mx + c \\ \ln k = (- \frac{E_{a}}{RT}) (\frac{1}{T}) + \ln A \end{aligned}$

CHXII04:CHEMICAL KINETICS

320243 The activation energy for a chemical reaction mainly depends upon

1 Temperature

2 Nature of reacting species

3 Concentration of the reacting species

4 Collision frequency

Explanation:

$E_{a}$ depends on bond energy of reactant.

CHXII04:CHEMICAL KINETICS

320239 The minimum energy required for a reaction to take place is called

1 Internal energy

2 Threshold energy

3 Activation energy

4 Free energy

CHXII04:CHEMICAL KINETICS

320240 Which among the following equation represents Arrhenius equation?

1

{k = A}_{e}^{E_{a} / R T}

2

k = A . e^{R T / E_{a}}

3

k = \frac{A}{e^{E_{a} / R T}}

4

k = \frac{A}{e^{R T / E_{a}}}

Explanation:

Variation of rate constant $k$ with temperature $T (K)$ is given by Arrhenius equation.
It is based on the two theories of reaction rates, i.e., collision theory and transition state theory.
$k = A e^{- E_{a} / R T} = \frac{A}{e^{E a / R T}} (1)$
where ' $A$ ' is called the frequency factor or the pre-exponential factor.
$E_{a}$ is activation energy $e^{- E_{a} / R T}$ is referred as Boltzmann factor. A, has same unit as the rate constant. Collectively $A$ and $E_{a}$ are called the Arrhenius parameters of the reaction.

CHXII04:CHEMICAL KINETICS

320241 A reactant (1) forms two products

$A \overset{k_{1}}{\to} B$ , Activation energy $E_{a_{1}}$

$A \overset{k_{2}}{\to} C$ , Activation energy $E_{a_{2}}$

If ${(E_{a})}_{2} = 2 {(E_{a})}_{1}$ then $k_{1} and k_{2}$ are related as

1

k_{2} = k_{1} e^{E_{a_{2}} /RT}

2

k_{1} = k_{2} e^{E_{a_{1}} /RT}

3

k_{1} = A k_{2} e^{E_{a_{1}} /RT}

4

k_{1} = 2 k_{2} e^{E_{a_{2}} /RT}

Explanation:

$A \overset{k_{1}}{⟶} B, A \overset{k_{2}}{⟶} C$
By Arrhenius equation,
$\begin{aligned} k_{1} = A^{'} e^{- E_{α_{l}} / R T} \\ ∴ E_{a_{2}} = 2 E_{a_{1}} \\ ∴ k_{2} = A^{'} e^{- E_{a_{1}} / R T} \\ \frac{k_{1}}{k_{2}} = \frac{A^{'} e^{- E_{q_{1}} / R T}}{A^{'} e^{- E_{α_{2}} / R T}} = e^{E_{q_{1}} / R T} \\ ∴ k_{1} = k_{2} e^{E_{q /} / R T} \end{aligned}$
and $k_{2} = A^{'} e^{- E_{q_{2}} / R T} [A^{'}$ is Arrhenius constant $]$

CHXII04:CHEMICAL KINETICS

320242 Which plots will give the value of activation energy?

1 k Vs T

2

1 / k V s T

3

l n k V s T

4

l n k V s 1 / T

Explanation:

According to Arrhenius equation,
$k = {Ae}^{- E_{a} / RT} \Rightarrow \ln k = \ln A - \frac{E_{a}}{RT}$
Rearrange the above equation in the form of
$\begin{aligned} y = mx + c \\ \ln k = (- \frac{E_{a}}{RT}) (\frac{1}{T}) + \ln A \end{aligned}$

CHXII04:CHEMICAL KINETICS

320243 The activation energy for a chemical reaction mainly depends upon

1 Temperature

2 Nature of reacting species

3 Concentration of the reacting species

4 Collision frequency

Explanation:

$E_{a}$ depends on bond energy of reactant.

CHXII04:CHEMICAL KINETICS

320239 The minimum energy required for a reaction to take place is called

1 Internal energy

2 Threshold energy

3 Activation energy

4 Free energy

CHXII04:CHEMICAL KINETICS

320240 Which among the following equation represents Arrhenius equation?

1

{k = A}_{e}^{E_{a} / R T}

2

k = A . e^{R T / E_{a}}

3

k = \frac{A}{e^{E_{a} / R T}}

4

k = \frac{A}{e^{R T / E_{a}}}

Explanation:

Variation of rate constant $k$ with temperature $T (K)$ is given by Arrhenius equation.
It is based on the two theories of reaction rates, i.e., collision theory and transition state theory.
$k = A e^{- E_{a} / R T} = \frac{A}{e^{E a / R T}} (1)$
where ' $A$ ' is called the frequency factor or the pre-exponential factor.
$E_{a}$ is activation energy $e^{- E_{a} / R T}$ is referred as Boltzmann factor. A, has same unit as the rate constant. Collectively $A$ and $E_{a}$ are called the Arrhenius parameters of the reaction.

CHXII04:CHEMICAL KINETICS

320241 A reactant (1) forms two products

$A \overset{k_{1}}{\to} B$ , Activation energy $E_{a_{1}}$

$A \overset{k_{2}}{\to} C$ , Activation energy $E_{a_{2}}$

If ${(E_{a})}_{2} = 2 {(E_{a})}_{1}$ then $k_{1} and k_{2}$ are related as

1

k_{2} = k_{1} e^{E_{a_{2}} /RT}

2

k_{1} = k_{2} e^{E_{a_{1}} /RT}

3

k_{1} = A k_{2} e^{E_{a_{1}} /RT}

4

k_{1} = 2 k_{2} e^{E_{a_{2}} /RT}

Explanation:

$A \overset{k_{1}}{⟶} B, A \overset{k_{2}}{⟶} C$
By Arrhenius equation,
$\begin{aligned} k_{1} = A^{'} e^{- E_{α_{l}} / R T} \\ ∴ E_{a_{2}} = 2 E_{a_{1}} \\ ∴ k_{2} = A^{'} e^{- E_{a_{1}} / R T} \\ \frac{k_{1}}{k_{2}} = \frac{A^{'} e^{- E_{q_{1}} / R T}}{A^{'} e^{- E_{α_{2}} / R T}} = e^{E_{q_{1}} / R T} \\ ∴ k_{1} = k_{2} e^{E_{q /} / R T} \end{aligned}$
and $k_{2} = A^{'} e^{- E_{q_{2}} / R T} [A^{'}$ is Arrhenius constant $]$

CHXII04:CHEMICAL KINETICS

320242 Which plots will give the value of activation energy?

1 k Vs T

2

1 / k V s T

3

l n k V s T

4

l n k V s 1 / T

Explanation:

According to Arrhenius equation,
$k = {Ae}^{- E_{a} / RT} \Rightarrow \ln k = \ln A - \frac{E_{a}}{RT}$
Rearrange the above equation in the form of
$\begin{aligned} y = mx + c \\ \ln k = (- \frac{E_{a}}{RT}) (\frac{1}{T}) + \ln A \end{aligned}$

CHXII04:CHEMICAL KINETICS

320243 The activation energy for a chemical reaction mainly depends upon

1 Temperature

2 Nature of reacting species

3 Concentration of the reacting species

4 Collision frequency

Explanation:

$E_{a}$ depends on bond energy of reactant.

CHXII04:CHEMICAL KINETICS

320239 The minimum energy required for a reaction to take place is called

1 Internal energy

2 Threshold energy

3 Activation energy

4 Free energy

CHXII04:CHEMICAL KINETICS

320240 Which among the following equation represents Arrhenius equation?

1

{k = A}_{e}^{E_{a} / R T}

2

k = A . e^{R T / E_{a}}

3

k = \frac{A}{e^{E_{a} / R T}}

4

k = \frac{A}{e^{R T / E_{a}}}

Explanation:

Variation of rate constant $k$ with temperature $T (K)$ is given by Arrhenius equation.
It is based on the two theories of reaction rates, i.e., collision theory and transition state theory.
$k = A e^{- E_{a} / R T} = \frac{A}{e^{E a / R T}} (1)$
where ' $A$ ' is called the frequency factor or the pre-exponential factor.
$E_{a}$ is activation energy $e^{- E_{a} / R T}$ is referred as Boltzmann factor. A, has same unit as the rate constant. Collectively $A$ and $E_{a}$ are called the Arrhenius parameters of the reaction.

CHXII04:CHEMICAL KINETICS

320241 A reactant (1) forms two products

$A \overset{k_{1}}{\to} B$ , Activation energy $E_{a_{1}}$

$A \overset{k_{2}}{\to} C$ , Activation energy $E_{a_{2}}$

If ${(E_{a})}_{2} = 2 {(E_{a})}_{1}$ then $k_{1} and k_{2}$ are related as

1

k_{2} = k_{1} e^{E_{a_{2}} /RT}

2

k_{1} = k_{2} e^{E_{a_{1}} /RT}

3

k_{1} = A k_{2} e^{E_{a_{1}} /RT}

4

k_{1} = 2 k_{2} e^{E_{a_{2}} /RT}

Explanation:

$A \overset{k_{1}}{⟶} B, A \overset{k_{2}}{⟶} C$
By Arrhenius equation,
$\begin{aligned} k_{1} = A^{'} e^{- E_{α_{l}} / R T} \\ ∴ E_{a_{2}} = 2 E_{a_{1}} \\ ∴ k_{2} = A^{'} e^{- E_{a_{1}} / R T} \\ \frac{k_{1}}{k_{2}} = \frac{A^{'} e^{- E_{q_{1}} / R T}}{A^{'} e^{- E_{α_{2}} / R T}} = e^{E_{q_{1}} / R T} \\ ∴ k_{1} = k_{2} e^{E_{q /} / R T} \end{aligned}$
and $k_{2} = A^{'} e^{- E_{q_{2}} / R T} [A^{'}$ is Arrhenius constant $]$

CHXII04:CHEMICAL KINETICS

320242 Which plots will give the value of activation energy?

1 k Vs T

2

1 / k V s T

3

l n k V s T

4

l n k V s 1 / T

Explanation:

According to Arrhenius equation,
$k = {Ae}^{- E_{a} / RT} \Rightarrow \ln k = \ln A - \frac{E_{a}}{RT}$
Rearrange the above equation in the form of
$\begin{aligned} y = mx + c \\ \ln k = (- \frac{E_{a}}{RT}) (\frac{1}{T}) + \ln A \end{aligned}$

CHXII04:CHEMICAL KINETICS

320243 The activation energy for a chemical reaction mainly depends upon

1 Temperature

2 Nature of reacting species

3 Concentration of the reacting species

4 Collision frequency

Explanation:

$E_{a}$ depends on bond energy of reactant.

CHXII04:CHEMICAL KINETICS

320239 The minimum energy required for a reaction to take place is called

1 Internal energy

2 Threshold energy

3 Activation energy

4 Free energy

CHXII04:CHEMICAL KINETICS

320240 Which among the following equation represents Arrhenius equation?

1

{k = A}_{e}^{E_{a} / R T}

2

k = A . e^{R T / E_{a}}

3

k = \frac{A}{e^{E_{a} / R T}}

4

k = \frac{A}{e^{R T / E_{a}}}

Explanation:

Variation of rate constant $k$ with temperature $T (K)$ is given by Arrhenius equation.
It is based on the two theories of reaction rates, i.e., collision theory and transition state theory.
$k = A e^{- E_{a} / R T} = \frac{A}{e^{E a / R T}} (1)$
where ' $A$ ' is called the frequency factor or the pre-exponential factor.
$E_{a}$ is activation energy $e^{- E_{a} / R T}$ is referred as Boltzmann factor. A, has same unit as the rate constant. Collectively $A$ and $E_{a}$ are called the Arrhenius parameters of the reaction.

CHXII04:CHEMICAL KINETICS

320241 A reactant (1) forms two products

$A \overset{k_{1}}{\to} B$ , Activation energy $E_{a_{1}}$

$A \overset{k_{2}}{\to} C$ , Activation energy $E_{a_{2}}$

If ${(E_{a})}_{2} = 2 {(E_{a})}_{1}$ then $k_{1} and k_{2}$ are related as

1

k_{2} = k_{1} e^{E_{a_{2}} /RT}

2

k_{1} = k_{2} e^{E_{a_{1}} /RT}

3

k_{1} = A k_{2} e^{E_{a_{1}} /RT}

4

k_{1} = 2 k_{2} e^{E_{a_{2}} /RT}

Explanation:

$A \overset{k_{1}}{⟶} B, A \overset{k_{2}}{⟶} C$
By Arrhenius equation,
$\begin{aligned} k_{1} = A^{'} e^{- E_{α_{l}} / R T} \\ ∴ E_{a_{2}} = 2 E_{a_{1}} \\ ∴ k_{2} = A^{'} e^{- E_{a_{1}} / R T} \\ \frac{k_{1}}{k_{2}} = \frac{A^{'} e^{- E_{q_{1}} / R T}}{A^{'} e^{- E_{α_{2}} / R T}} = e^{E_{q_{1}} / R T} \\ ∴ k_{1} = k_{2} e^{E_{q /} / R T} \end{aligned}$
and $k_{2} = A^{'} e^{- E_{q_{2}} / R T} [A^{'}$ is Arrhenius constant $]$

CHXII04:CHEMICAL KINETICS

320242 Which plots will give the value of activation energy?

1 k Vs T

2

1 / k V s T

3

l n k V s T

4

l n k V s 1 / T

Explanation:

According to Arrhenius equation,
$k = {Ae}^{- E_{a} / RT} \Rightarrow \ln k = \ln A - \frac{E_{a}}{RT}$
Rearrange the above equation in the form of
$\begin{aligned} y = mx + c \\ \ln k = (- \frac{E_{a}}{RT}) (\frac{1}{T}) + \ln A \end{aligned}$

CHXII04:CHEMICAL KINETICS

320243 The activation energy for a chemical reaction mainly depends upon

1 Temperature

2 Nature of reacting species

3 Concentration of the reacting species

4 Collision frequency

Explanation:

$E_{a}$ depends on bond energy of reactant.