Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

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Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

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(N/A) The combustion of fuels is a chemical reaction that requires a certain minimum amount of energy,known as the activation energy $(E_a)$,to initiate the process. At room temperature,the average kinetic energy of the fuel molecules is significantly lower than the required activation energy. Therefore,the molecules do not possess sufficient energy to overcome the energy barrier,and the reaction does not occur spontaneously.

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Class 12

Chemistry Questions

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

Activation energy $(E_a)$ and rate constants $(k_1)$ and $(k_2)$ of a chemical reaction at two different temperatures $(T_1)$ and $(T_2)$ are related by

MediumAIPMT 2012

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For a first-order reaction at $300 \, ^\circ C$,the activation energy is $35 \, kcal \, mol^{-1}$ and the frequency factor is $1.45 \times 10^{11} \, s^{-1}$. Calculate the rate constant.

Medium

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The temperature dependence of the rate constant $k$ is expressed as $k = A e^{-E_a / RT}$. When a plot between $\log k$ and $1/T$ is plotted,we get the graph as shown. What is the value of the slope in the graph?

Medium

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Reactant $A$ converts to product $D$ through the given mechanism (with the net evolution of heat) :
$A \rightarrow B$ $slow ; \Delta H=+ve$
$B \rightarrow C$ $fast ; \Delta H=-ve$
$C \rightarrow D$ $fast ; \Delta H=-ve$

Which of the following represents the above reaction mechanism ?

DifficultJEE MAIN 2025

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The time required for $10 \%$ completion of a first order reaction at $298 \,K$ is equal to that required for its $25 \%$ completion at $308 \,K$. If the value of $A$ is $4 \times 10^{10} \,s^{-1}$,calculate $k$ at $318 \,K$ and $E_a$.

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$A \rightarrow B$	$slow ; \Delta H=+ve$
$B \rightarrow C$	$fast ; \Delta H=-ve$
$C \rightarrow D$	$fast ; \Delta H=-ve$

Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

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Activation energy $(E_a)$ and rate constants $(k_1)$ and $(k_2)$ of a chemical reaction at two different temperatures $(T_1)$ and $(T_2)$ are related by

For a first-order reaction at $300 \, ^\circ C$,the activation energy is $35 \, kcal \, mol^{-1}$ and the frequency factor is $1.45 \times 10^{11} \, s^{-1}$. Calculate the rate constant.

The temperature dependence of the rate constant $k$ is expressed as $k = A e^{-E_a / RT}$. When a plot between $\log k$ and $1/T$ is plotted,we get the graph as shown. What is the value of the slope in the graph?

Reactant $A$ converts to product $D$ through the given mechanism (with the net evolution of heat) :$A \rightarrow B$$slow ; \Delta H=+ve$$B \rightarrow C$$fast ; \Delta H=-ve$$C \rightarrow D$$fast ; \Delta H=-ve$Which of the following represents the above reaction mechanism ?

The time required for $10 \%$ completion of a first order reaction at $298 \,K$ is equal to that required for its $25 \%$ completion at $308 \,K$. If the value of $A$ is $4 \times 10^{10} \,s^{-1}$,calculate $k$ at $318 \,K$ and $E_a$.

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Reactant $A$ converts to product $D$ through the given mechanism (with the net evolution of heat) :
$A \rightarrow B$ $slow ; \Delta H=+ve$
$B \rightarrow C$ $fast ; \Delta H=-ve$
$C \rightarrow D$ $fast ; \Delta H=-ve$

Which of the following represents the above reaction mechanism ?