Which of the following is the energy threshold that must be overcome in order for collisions to be successful?
Activated complex
Activation energy
Enthalpy change
What is the enthalpy change for the forward reaction shown by the reaction pathway in the graph below?
-100 kJ mol-1
+100 kJ mol-1
+50 kJ mol-1
What effect would the use of a catalyst have on a chemical reaction?
Activation energy remains unchanged; enthalpy increases
Activation energy increases; enthalpy unchanged
Activation energy decreases; enthalpy unchanged
Which of the following factors would not increase the number of collisions between reactant molecules?
Increasing the particle size of the reaction
Increasing the temperature of the reaction
Increasing the concentration of the reaction
What is the main reason that a small increase in the temperature of a reaction mixture results in a large increase in the rate of the reaction?
The activation energy is lowered
The enthalpy change is decreased
The kinetic energy of the particles has increased
What is the activation energy for the reverse reaction represented by the reaction pathway in the graph below?
A
B
C
Using the reaction pathway shown in the graph below, calculate the activation energy for the forwards reaction.
10 kJ mol-1
-20 kJ mol-1
30 kJ mol-1
What is the name given to a high energy intermediate state that is established when bonds inside the reactant molecules are breaking and new bonds are being formed?
Exothermic reaction
Which of the following collisions is most likely to result in a successful reaction?
Which area(s) of the following graph represent the molecules that have enough kinetic energy to react at the higher temperature (T2)?
A, B + C
B + C