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The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol–1. The ratio of rate constant to the Arrhenius factor is
Correct answer is '0.1'. Can you explain this answer?
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The activation energy of a reaction at a given temperature is found to...
-1. This means that the minimum amount of energy required for the reaction to occur is 2.303 RT J/mol.
In other words, molecules need to have a certain amount of energy in order to react, and this energy is known as the activation energy. If the energy of the molecules is below the activation energy, they will not react, but if it is above the activation energy, they will react and form products.
The activation energy is dependent on the specific reaction and the temperature at which it occurs. As the temperature increases, the average energy of the molecules also increases, making it more likely that they will have enough energy to overcome the activation energy barrier and react.
Knowing the activation energy of a reaction is important in understanding and optimizing chemical reactions, such as in the development of more efficient and sustainable industrial processes.
In other words, molecules need to have a certain amount of energy in order to react, and this energy is known as the activation energy. If the energy of the molecules is below the activation energy, they will not react, but if it is above the activation energy, they will react and form products.
The activation energy is dependent on the specific reaction and the temperature at which it occurs. As the temperature increases, the average energy of the molecules also increases, making it more likely that they will have enough energy to overcome the activation energy barrier and react.
Knowing the activation energy of a reaction is important in understanding and optimizing chemical reactions, such as in the development of more efficient and sustainable industrial processes.
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The activation energy of a reaction at a given temperature is found to...
K=Ae^(-Ea/RT), K/A=10^(-Ea/2.303RT), now put the value of activation energy, k/A=10^-1 , so, k/A=0.1
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The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol–1.The ratio of rate constant to the Arrhenius factor isCorrect answer is '0.1'. Can you explain this answer?
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