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The rate of a chemical reaction doubles for every 10ºC rise of temperature. If the temperature is raised by 50ºC, the rate of the reaction increases by about :
[AIEEE 2011]
- a)24 times
- b)32 times
- c)64 times
- d)10 times
Correct answer is option 'B'. Can you explain this answer?
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The rate of a chemical reaction doubles for every 10ºC rise of te...
The correct answer is Option B.
For every 10 °C rise of temperature, the rate is doubled. Thus, temperature coefficient of the reaction =2
When temperature is increased by 50°, rate becomes = 2(50/10)
= 25 times
= 32
For every 10 °C rise of temperature, the rate is doubled. Thus, temperature coefficient of the reaction =2
When temperature is increased by 50°, rate becomes = 2(50/10)
= 25 times
= 32
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The rate of a chemical reaction doubles for every 10ºC rise of te...
The rate of a chemical reaction doubling for every 10 units of a particular variable is known as the "rate constant" or "reaction constant." This is a concept derived from the Arrhenius equation, which relates the rate of a chemical reaction to the temperature and activation energy.
In general, the rate constant is given by the equation:
k = A * e^(-Ea/RT)
where:
- k is the rate constant
- A is the pre-exponential factor (also known as the collision frequency factor), which represents the frequency of successful collisions between reactant molecules
- Ea is the activation energy, which is the minimum energy required for a reaction to occur
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
According to the Arrhenius equation, increasing the temperature (T) will increase the rate constant (k), leading to a faster reaction rate. The relationship between temperature and rate constant is exponential, meaning that a small increase in temperature can lead to a significant increase in reaction rate.
If the rate of a chemical reaction doubles for every 10 units of a particular variable, it means that the rate constant (k) doubles when the variable increases by 10 units. This indicates a strong dependence of the reaction rate on that variable.
In general, the rate constant is given by the equation:
k = A * e^(-Ea/RT)
where:
- k is the rate constant
- A is the pre-exponential factor (also known as the collision frequency factor), which represents the frequency of successful collisions between reactant molecules
- Ea is the activation energy, which is the minimum energy required for a reaction to occur
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
According to the Arrhenius equation, increasing the temperature (T) will increase the rate constant (k), leading to a faster reaction rate. The relationship between temperature and rate constant is exponential, meaning that a small increase in temperature can lead to a significant increase in reaction rate.
If the rate of a chemical reaction doubles for every 10 units of a particular variable, it means that the rate constant (k) doubles when the variable increases by 10 units. This indicates a strong dependence of the reaction rate on that variable.
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The rate of a chemical reaction doubles for every 10ºC rise of temperature. If the temperature is raised by 50ºC, the rate of the reaction increases by about :[AIEEE 2011]a)24 timesb)32 timesc)64 timesd)10 timesCorrect answer is option 'B'. Can you explain this answer?
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