If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
Practice Questions
1 question
Q1
If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
Rate constant decreases
Rate constant remains the same
Rate constant increases
Rate constant doubles
According to the Arrhenius equation, an increase in temperature generally increases the rate constant, as it provides more energy to overcome the activation energy barrier.
Questions & Step-by-step Solutions
1 item
Q
Q: If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
Solution: According to the Arrhenius equation, an increase in temperature generally increases the rate constant, as it provides more energy to overcome the activation energy barrier.
Steps: 6
Step 1: Understand what activation energy is. It is the minimum energy required for a reaction to occur.
Step 2: Know that the rate constant (k) of a reaction is influenced by temperature.
Step 3: Familiarize yourself with the Arrhenius equation, which shows the relationship between temperature and the rate constant.
Step 4: Recognize that increasing the temperature from 300 K to 350 K means the molecules have more energy.
Step 5: Realize that with more energy, more molecules can overcome the activation energy barrier.
Step 6: Conclude that as a result, the rate constant (k) will increase when the temperature is raised.
