EXERCISE 1. Describe the effect of each of the following on the rate of the reaction of:
a) magnesium metal with a solution of hydrochloric acid
b) the molarity of the hydrochloric acid
C) the temperature of the solution
d) the size of the pieces of magnesium.
2. For each of the following situations, state whether the rate of the reaction
would increase or decrease, and explain your answer using the collision theory.
a) The concentration of a reactant is doubled.
b) The reaction is moved from a lab bench at room temperature into an ice
bath.
c) A solid crystalline reactant is broken down into smaller pieces with a
hammer.​