For a reaction with an activation energy of 50 kJ/mol, what will happen to the r
Practice Questions
Q1
For a reaction with an activation energy of 50 kJ/mol, what will happen to the rate if the temperature is increased by 20°C? (2022)
Rate decreases
Rate remains the same
Rate increases significantly
Rate increases slightly
Questions & Step-by-Step Solutions
For a reaction with an activation energy of 50 kJ/mol, what will happen to the rate if the temperature is increased by 20°C? (2022)
Step 1: Understand that activation energy is the minimum energy required for a reaction to occur.
Step 2: Recognize that increasing the temperature gives molecules more kinetic energy.
Step 3: Realize that with more kinetic energy, more molecules can overcome the activation energy barrier.
Step 4: Conclude that as a result, the rate of the reaction will increase when the temperature is raised by 20°C.
Activation Energy – The minimum energy required for a chemical reaction to occur.
Effect of Temperature on Reaction Rate – Increasing temperature typically increases the kinetic energy of molecules, leading to a higher reaction rate.
Arrhenius Equation – A formula that shows the relationship between temperature and the rate constant of a reaction, indicating that rate increases exponentially with temperature.
