chemistry: rate of reactions

• rate graphs: a graph is used to follow the course of reaction. comparing the graphs show the differences in the rates of similar reactions. The steeper the line is the faster the reaction showing that it could have had something to affect the rate of reactions.
• catalyst: lowers the activation energy of the reaction. a catalyst is a substance that speeds up a chemical reaction without being used up in the reaction. by lowering the activation energy it increases the chance of a successful collisions.
• surface area: breaking a solid into smaller pieces increases the surface area. a larger surface area provides more space for the reacting particles to collide, this increases the chance of successful collisions.
• concentration: increasing the concentration increases the number of particles . at a higher pressure there are more reacting particles in the same space, increases the chance of successful collisions
• temperature: increasing temperature makes particles move faster. at a higher temperature the particles have more kinetic energy and move faster, this increases the chance of successful collisions
• activation energy: the activation energy is the minimum amount of energy needed for a reaction to occur
• collision theory: for a reaction to happen they must successfully collide. a successful reaction is one that leads to a reaction happening a successful collision happens when the reacting particles have the sufficient energy. increasing the rate of reaction increases the frequency of successful collisions. there are four ways to change the rate of reaction: temperature, surface area, concentration and using a catalyst.
• how to measure rates of reactions: capture and measure the volume of gas produced over time. measure and record the change in mass. measure and record the amount of light passing through a chemical reaction ( producing a precipitate )