If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?
Practice Questions
1 question
Q1
If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?
20 kJ/mol
40 kJ/mol
60 kJ/mol
80 kJ/mol
Using the Arrhenius equation, a rule of thumb states that for every 10°C increase in temperature, the rate doubles if Ea is around 40 kJ/mol.
Questions & Step-by-step Solutions
1 item
Q
Q: If the rate of a reaction doubles when the temperature is increased by 10°C, what is the approximate activation energy (Ea) of the reaction?
Solution: Using the Arrhenius equation, a rule of thumb states that for every 10°C increase in temperature, the rate doubles if Ea is around 40 kJ/mol.
Steps: 5
Step 1: Understand that the rate of a reaction can change with temperature.
Step 2: Know that the Arrhenius equation relates temperature and reaction rate to activation energy (Ea).
Step 3: Recognize the rule of thumb: if the rate doubles with a 10°C increase, it suggests a specific activation energy.
Step 4: Remember that for an activation energy of around 40 kJ/mol, the rate will double with a 10°C increase.
Step 5: Conclude that the approximate activation energy (Ea) of the reaction is 40 kJ/mol.
