Illustrated in the plot is the energy change during a chemical reaction.
How many transition states exist in this reaction?
How many intermediates exist in this reaction?
Estimate, to the nearest 5 kJ/mol, the activation energy for the forward reaction.
The reaction profile can be altered by changing the conditions under which the reaction takes place. For which of the following reaction profiles is the activation energy for the forward reaction lowest?
When the products of a chemical reaction are more energetically stable than the reactants, energy is released as heat. What is the type of this described reaction?
Fill in the blank: In a chemical reaction, a high-energy transition state must be reached for chemical bonds to be broken and for products to be formed. The amount of energy needed to reach this transition state is known as the .