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The rate of a reaction triple when temperature changes from 20°C to 50°C. Calculate energy (J/mol) of activation for the reaction (R = 8.314 JK–1 mol–1). [rounded up to first decimal place]
Correct answer is between '28810,28830'. Can you explain this answer?
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The rate of a reaction triple when temperature changes from 20°C t...
°C to 60°C. This is an example of:
The rate of a reaction is strongly influenced by temperature. The increase in temperature causes an increase in the average kinetic energy of the reacting molecules, which in turn increases the frequency of collisions between the reacting species. This leads to a higher probability of successful collisions, resulting in an increase in reaction rate.
The relationship between reaction rate and temperature can be described by the Arrhenius equation:
k = A * e^(-Ea/RT)
where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the absolute temperature.
From this equation, we can see that an increase in temperature will increase the rate constant, and therefore increase the reaction rate. The exact relationship between rate and temperature depends on the activation energy and pre-exponential factor, but in general, a change in temperature of 10°C will result in a change in reaction rate of approximately 2-3 times.
In this case, the rate of the reaction tripled when temperature changed from 20°C to 60°C. This indicates that the activation energy and pre-exponential factor are such that a 40°C increase in temperature results in a 3-fold increase in reaction rate.
The rate of a reaction is strongly influenced by temperature. The increase in temperature causes an increase in the average kinetic energy of the reacting molecules, which in turn increases the frequency of collisions between the reacting species. This leads to a higher probability of successful collisions, resulting in an increase in reaction rate.
The relationship between reaction rate and temperature can be described by the Arrhenius equation:
k = A * e^(-Ea/RT)
where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the absolute temperature.
From this equation, we can see that an increase in temperature will increase the rate constant, and therefore increase the reaction rate. The exact relationship between rate and temperature depends on the activation energy and pre-exponential factor, but in general, a change in temperature of 10°C will result in a change in reaction rate of approximately 2-3 times.
In this case, the rate of the reaction tripled when temperature changed from 20°C to 60°C. This indicates that the activation energy and pre-exponential factor are such that a 40°C increase in temperature results in a 3-fold increase in reaction rate.
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The rate of a reaction triple when temperature changes from 20°C t...
Bhaiya use Arrhenius equation na.
and get the answer na.
and get the answer na.
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The rate of a reaction triple when temperature changes from 20°C to 50°C. Calculate energy (J/mol) of activation for the reaction (R = 8.314 JK–1 mol–1). [rounded up to first decimal place]Correct answer is between '28810,28830'. Can you explain this answer?
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