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The rate of chemical reaction is doubled for every 10oC rise in temperature because of
- a)increase in the activation energy
- b)decrease in the activation energy
- c)increase in the number of molecular collision
- d)increase in the number of activated molecules
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
The rate of chemical reaction is doubled for every 10oC rise in temper...
Explanation:
- Increase in Temperature: When the temperature of a system is increased, the kinetic energy of the molecules also increases. This leads to a greater number of molecules having energy equal to or greater than the activation energy required for the reaction to occur.
- Number of Activated Molecules: With the increase in temperature, the number of molecules that have enough energy to overcome the activation energy barrier also increases. This results in more collisions between these activated molecules, leading to a higher rate of reaction.
- Rate of Reaction Doubling: For many chemical reactions, the rate of reaction approximately doubles for every 10oC rise in temperature. This is due to the exponential relationship between temperature and reaction rate, as described by the Arrhenius equation.
- Activation Energy: The activation energy is the minimum amount of energy required for a reaction to occur. With an increase in temperature, the number of molecules with energy equal to or greater than the activation energy increases, leading to a higher rate of reaction.
- Conclusion: Therefore, the rate of chemical reaction is doubled for every 10oC rise in temperature primarily because of the increase in the number of activated molecules, resulting in more collisions and a higher likelihood of successful reactions taking place.
- Increase in Temperature: When the temperature of a system is increased, the kinetic energy of the molecules also increases. This leads to a greater number of molecules having energy equal to or greater than the activation energy required for the reaction to occur.
- Number of Activated Molecules: With the increase in temperature, the number of molecules that have enough energy to overcome the activation energy barrier also increases. This results in more collisions between these activated molecules, leading to a higher rate of reaction.
- Rate of Reaction Doubling: For many chemical reactions, the rate of reaction approximately doubles for every 10oC rise in temperature. This is due to the exponential relationship between temperature and reaction rate, as described by the Arrhenius equation.
- Activation Energy: The activation energy is the minimum amount of energy required for a reaction to occur. With an increase in temperature, the number of molecules with energy equal to or greater than the activation energy increases, leading to a higher rate of reaction.
- Conclusion: Therefore, the rate of chemical reaction is doubled for every 10oC rise in temperature primarily because of the increase in the number of activated molecules, resulting in more collisions and a higher likelihood of successful reactions taking place.
Most Upvoted Answer
The rate of chemical reaction is doubled for every 10oC rise in temper...
Explanation:
The rate of a chemical reaction is the measure of how fast the reactants are converted into products. The rate of a chemical reaction is influenced by various factors, including temperature, concentration of reactants, surface area, and catalysts.
Effect of Temperature on Rate of Chemical Reaction:
Temperature is one of the critical factors that affect the rate of a chemical reaction. The rate of a chemical reaction increases with an increase in temperature. This is because the kinetic energy of the molecules increases with increasing temperature. Higher kinetic energy means that molecules move faster and collide more frequently with each other with greater force.
The Arrhenius equation describes the relationship between temperature and reaction rate. It states that the rate constant (k) of a reaction is proportional to the exponential factor of the activation energy (Ea) divided by the product of the Boltzmann constant (k) and the temperature (T).
k = Ae^(-Ea/RT)
Where A is the pre-exponential factor, R is the gas constant, and T is the temperature in kelvin.
Doubling of Rate of Reaction with Every 10oC Increase in Temperature:
The Arrhenius equation explains why the rate of a chemical reaction is doubled for every 10oC rise in temperature. This relationship can be derived from the equation by taking the ratio of two rate constants at different temperatures.
k2/k1 = (Ae^(-Ea/RT2))/(Ae^(-Ea/RT1))
k2/k1 = e^(Ea/R)((1/T1)-(1/T2))
If we take T2 = T1 + 10oC, then the ratio becomes:
k2/k1 = e^(Ea/R)(1/T1 - 1/(T1+10))
Simplifying the equation gives:
k2/k1 = 2
This means that the rate of a chemical reaction is doubled for every 10oC rise in temperature.
Reason for Doubling of Rate of Reaction:
The doubling of the rate of a chemical reaction with every 10oC increase in temperature is due to the increase in the number of activated molecules. At higher temperatures, a larger number of molecules have sufficient energy to overcome the activation energy barrier and participate in the reaction. This leads to an increase in the rate of the reaction.
The rate of a chemical reaction is the measure of how fast the reactants are converted into products. The rate of a chemical reaction is influenced by various factors, including temperature, concentration of reactants, surface area, and catalysts.
Effect of Temperature on Rate of Chemical Reaction:
Temperature is one of the critical factors that affect the rate of a chemical reaction. The rate of a chemical reaction increases with an increase in temperature. This is because the kinetic energy of the molecules increases with increasing temperature. Higher kinetic energy means that molecules move faster and collide more frequently with each other with greater force.
The Arrhenius equation describes the relationship between temperature and reaction rate. It states that the rate constant (k) of a reaction is proportional to the exponential factor of the activation energy (Ea) divided by the product of the Boltzmann constant (k) and the temperature (T).
k = Ae^(-Ea/RT)
Where A is the pre-exponential factor, R is the gas constant, and T is the temperature in kelvin.
Doubling of Rate of Reaction with Every 10oC Increase in Temperature:
The Arrhenius equation explains why the rate of a chemical reaction is doubled for every 10oC rise in temperature. This relationship can be derived from the equation by taking the ratio of two rate constants at different temperatures.
k2/k1 = (Ae^(-Ea/RT2))/(Ae^(-Ea/RT1))
k2/k1 = e^(Ea/R)((1/T1)-(1/T2))
If we take T2 = T1 + 10oC, then the ratio becomes:
k2/k1 = e^(Ea/R)(1/T1 - 1/(T1+10))
Simplifying the equation gives:
k2/k1 = 2
This means that the rate of a chemical reaction is doubled for every 10oC rise in temperature.
Reason for Doubling of Rate of Reaction:
The doubling of the rate of a chemical reaction with every 10oC increase in temperature is due to the increase in the number of activated molecules. At higher temperatures, a larger number of molecules have sufficient energy to overcome the activation energy barrier and participate in the reaction. This leads to an increase in the rate of the reaction.
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The rate of chemical reaction is doubled for every 10oC rise in temperature because ofa)increase in the activation energyb)decrease in the activation energyc)increase in the number of molecular collisiond)increase in the number of activated moleculesCorrect answer is option 'D'. Can you explain this answer?
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