EVERYDAY SCIENCE

Detailed explanation-1: -Increasing the surface area of a reactant (by breaking a solid reactant into smaller particles) increases the number of particles available for collision and will increase the number of collisions between reactants per unit time.

Detailed explanation-2: -If one of the reactants is a solid, only the particles at the surface can partake in the reaction. Breaking the reactant into smaller pieces increases the surface and more particles are exposed to the reaction mixture. This results in an increased frequency of collisions and therefore a faster rate of reaction.

Detailed explanation-3: -If one of the reactants is a solid, the surface area of the solid will affect how fast the reaction goes. This is because the two types of molecule can only bump into each other at the liquid solid interface, i.e. on the surface of the solid. So the larger the surface area of the solid, the faster the reaction will be.

Detailed explanation-4: -The rate of a chemical reaction is affected by several parameters. Reactions involving two phases proceed more rapidly when there is greater surface area contact. If temperature or reactant concentration is increased, the rate of a given reaction generally increases as well.

Detailed explanation-5: -An increase in surface area increases the number of particles that come in contact with other reactant particles. As it exposes more reactant particles to the reaction it increases the frequency of collisions which increases the frequency of effective collisions resulting in a faster reaction rate.