For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?
Practice Questions
1 question
Q1
For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?
Rate constant decreases
Rate constant increases
Rate constant remains the same
Rate constant becomes zero
According to the Arrhenius equation, an increase in temperature results in an increase in the rate constant, k, as it provides more energy to overcome the activation energy barrier.
Questions & Step-by-step Solutions
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Q
Q: For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature on the rate constant?
Solution: According to the Arrhenius equation, an increase in temperature results in an increase in the rate constant, k, as it provides more energy to overcome the activation energy barrier.
Steps: 6
Step 1: Understand that the activation energy (Ea) is the energy needed for a reaction to occur.
Step 2: Know that the rate constant (k) is a number that tells us how fast a reaction happens.
Step 3: Learn about the Arrhenius equation, which shows the relationship between temperature and the rate constant: k = A * e^(-Ea/(RT)).
Step 4: Recognize that 'A' is a constant, 'R' is the gas constant, and 'T' is the temperature in Kelvin.
Step 5: Realize that as temperature (T) increases, the value of -Ea/(RT) becomes less negative, which makes e^(-Ea/(RT)) larger.
Step 6: Conclude that a larger value of e^(-Ea/(RT)) means a larger rate constant (k), indicating that the reaction will happen faster.
