When the surface area of a reactant increases, more particles are exposed to the other reactant, which increases the chance of collisions. This leads to more successful collisions per second, which increases the rate of reaction.
When the temperature of a chemical reaction increases, the average kinetic energy of the reactant molecules increases. This causes the molecules to move faster and collide with each other more often and with more energy.
Volume itself doesn't directly affect the rate of reaction, changes in volume can affect pressure and, in cases involving gaseous reactants, the equilibrium position, which can indirectly influence the rate of reaction.
A catalyst is a substance that speeds up a chemical reaction without being used up in the process. It does this by providing an alternative reaction pathway with a lower activation energy. This means that more reactant molecules can collide effectively, increasing the reaction rate.
There is an explanation video available below.
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