Practice Arrhenius Equation (3.5) - Unit 6: Chemical Kinetics

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6 sample questions

Question 1.
What does the Arrhenius equation express?
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Think about how these factors relate to reaction rates.
Question 2.
What is activation energy?
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Consider the energy barrier for chemical reactions.
3Question 3.
What is the form of the Arrhenius equation?
- k = A e^(-Ea/(RT))
- k = A + (Ea/RT)
- k = A * (T^Ea)
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Remember the exponential part!
4Question 4.
Does a lower activation energy lead to faster reactions?
- True
- False
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Consider the energy barrier concept.
Question 5.
Given that the activation energy (Ea) for a reaction is 75 kJ/mol, how would the rate constant (k) change if the temperature is increased from 298 K to 313 K?
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Calculate values using the exponential form of the Arrhenius equation.
Question 6.
If a catalyst decreases the activation energy from 100 kJ/mol to 70 kJ/mol, how will this affect the rate of reaction at a constant temperature of 298 K?
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Focus on how lowering Ea influences k.

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