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According to Arrhenius equation (K= rate constant and T= Temperature):
- a)In k decrease linearly 1/T
- b)In k decreases linearly T
- c)In k increases linearly with 1/T
- d)In k increases linearly with T
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
According to Arrhenius equation (K= rate constant and T= Temperature):...
Arrhenius equation is used for calculating the rate constant (k) of a chemical reaction. It relates the rate constant to the activation energy (Ea) and the temperature (T). The equation is given as:
k = A * e^(-Ea/RT)
where A is the pre-exponential factor, R is the gas constant, and e is the base of natural logarithm.
Effect of temperature on rate constant
The Arrhenius equation shows that the rate constant (k) is directly proportional to the temperature (T) and inversely proportional to the activation energy (Ea). Therefore, as the temperature increases, the rate of the reaction also increases.
Effect of temperature on activation energy
As the temperature increases, the activation energy decreases. This is because at higher temperatures, the molecules have more kinetic energy and are more likely to overcome the activation energy barrier and react.
Effect of temperature on k with respect to 1/T
Taking natural logarithm of both sides of the Arrhenius equation, we get:
ln k = ln A - (Ea/RT)
On rearranging, we get:
ln k = -(Ea/R) * (1/T) + ln A
This equation shows that the natural logarithm of the rate constant (ln k) decreases linearly with 1/T. Therefore, the correct answer is option 'A'.
Conclusion
In conclusion, the Arrhenius equation explains the effect of temperature on the rate constant of a chemical reaction. It shows that as the temperature increases, the rate of the reaction also increases. The equation also shows that the natural logarithm of the rate constant decreases linearly with 1/T.
k = A * e^(-Ea/RT)
where A is the pre-exponential factor, R is the gas constant, and e is the base of natural logarithm.
Effect of temperature on rate constant
The Arrhenius equation shows that the rate constant (k) is directly proportional to the temperature (T) and inversely proportional to the activation energy (Ea). Therefore, as the temperature increases, the rate of the reaction also increases.
Effect of temperature on activation energy
As the temperature increases, the activation energy decreases. This is because at higher temperatures, the molecules have more kinetic energy and are more likely to overcome the activation energy barrier and react.
Effect of temperature on k with respect to 1/T
Taking natural logarithm of both sides of the Arrhenius equation, we get:
ln k = ln A - (Ea/RT)
On rearranging, we get:
ln k = -(Ea/R) * (1/T) + ln A
This equation shows that the natural logarithm of the rate constant (ln k) decreases linearly with 1/T. Therefore, the correct answer is option 'A'.
Conclusion
In conclusion, the Arrhenius equation explains the effect of temperature on the rate constant of a chemical reaction. It shows that as the temperature increases, the rate of the reaction also increases. The equation also shows that the natural logarithm of the rate constant decreases linearly with 1/T.
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According to Arrhenius equation (K= rate constant and T= Temperature):a)In k decrease linearly 1/Tb)In k decreases linearly Tc)In k increases linearly with 1/Td)In k increases linearly with TCorrect answer is option 'A'. Can you explain this answer?
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