Factors -

Rate Of Reaction - Amount of product produced per unit time

Collision theory - for a chemical reaction to occur, the reactant particles must collide with sufficient energy and proper orientation.

• Concentration of the reactants in solution or the pressure of reacting gases
• Temperature at which the reaction is carried out
• Surface area of solid reactants
• The use of a catalyst

Graph Will Look Like -

Explanations -

• Concentration: Concentration Increased → More particles that can collide with each other → Increases frequency of collisions → Increased chances of particles colliding with the correct orientation and sufficient energy → Increases rate of reaction.
• Pressure - Pressure of reacting gases increased → Particles are forced closer together → More frequent collisions → Increased chances of particles colliding with the correct orientation and sufficient energy → Increased rate of reaction.
• Temperature: increase in temperature → increase in kinetic energy of particles → move faster and collide more frequently and energetically → Increased chances of particles colliding with the correct orientation and sufficient energy → higher rate of reaction
• Surface area: Increasing the surface area of a solid reactant by breaking it into smaller pieces or powder form → exposes more particles to the other reactants → Increased chances of particles colliding with the correct orientation and sufficient energy → increasing the frequency of collisions and the rate of reaction.
• Catalyst: A catalyst is a substance that lowers the activation energy required for a reaction to occur → Increased chances of particles colliding with sufficient energy → leading to an increased rate of reaction.

Setting Up Experiment -