Kinetics Flashcards
What is Activation Energy?
The min. amount of energy needed for a reaction to occur
What is the transition state?
Part of the reaction where some bonds are broken and some are made
What does the area under the graph show?
No. of particles
What happens to the curve when temperature is increased
The curve moves to the right and the peak is lower whilst the area under curve remains same and line for A.E sits higher
What effect does increasing pressure have on rate of reaction
Increase Rate of reaction as particles are closer together and collide more often. There are more frequent collisions and a higher chance of a reaction
what is a catalyst and what is its role
It is a substance that affect rates of reaction without being used up. It provides an alternate pathway that has a lower activation energy
What must happen in order for a chemical reaction to occur?
Reactants must physically collide with sufficient energy (the activation energy) to react and transfer electrons
How can you increase the rate of an aqueous reaction?
Increase the concentration so that there are an increased number of reactant molecules per unit and the frequency of collisions is increased
How can you increase the rate of a gaseous reaction?
Increase the pressure so that there are more reactant molecules per unit so that the frequency of collisions is increased
What is a homogeneous catalyst?
A catalyst In the same state/phase as the reactants
What is a heterogeneous catalyst?
A catalyst in a different state/phase as the reactants
What is Collision Theory?
A reaction will not take place between 2 particles unless they collide in the right direction with at least a certain min amount of kinetic energy
What does the peak of the curve represent?
Most likely energy of any single molecule
