Rates of Reaction

Question 1

Activation Energy

Answer 1

the minimum amount of energy needed for a reaction to happen

Question 2

Catalyst

Answer 2

speeds up a reaction without being used in the reaction itself, lowers the activation energy, causing a higher proportion of successful collisions

Question 3

Collision Theory

Answer 3

explains why rate of reaction changes, states that particles must collide before a reaction takes place and if there is a collision, it might take place, but not all collisions lead to reactions because they need energy in order to react, and reactants must have the activation energy in order to react

Question 4

Cocentration

Answer 4

increasing the particles per unit volume causes more frequent collisions

Question 5

Mean Rate of Reaction

Answer 5

quantity of reactant used / time or quantity of reactant formed / time

Question 6

Metabolism

Answer 6

the sum of all the reactions in the body

Question 7

Pressure

Answer 7

increasing the particles per unit volume causes more frequent collisions