Can someone please explain these? Thanks! Collision theory offers a simple expla
ID: 476246 • Letter: C
Question
Can someone please explain these? Thanks! Collision theory offers a simple explanation for how reactions occur-reading molecules must first collide. In order for colliding molecules to he converted into products, they must collide with enough energy and with a suitable orientation to break existing bonds in the reactants and form new bonds in the products. Any factor that changes either the total number of collisions or the average energy of the colliding molecules should affect the reaction rate. a) Using collision theory, predict how increasing the temperature should affect the rate of a chemical reaction. State the prediction in the form of a hypothesis and explain your reasoning. b) Using collision theory, predict how increasing the concentration of a reactant should affect the rate of a chemical reaction. State the prediction in the form of a hypothesis and explain your reasoning.Explanation / Answer
The collision theory states that when suitable particles of the reactant hit each other, only a certain percentage of the collisions cause any noticeable or significant chemical change; these successful changes are called successful collisions.
When you increase the temperature of a reaction, the kinetic energy of the molecules also increases as it is directly proportional to Temperature.
More Kinetic energy gives higher velocities and in turn more number of collisions of molecules. This increases the chance of having successful collisions . Hence, with increase in temperature the rate of reaction increases.
Similar is the case with concentration. When you increase conc., what you basically do is increase the no of molecules per unit volume of space. This is analogous to more no of people in the same area of the lift. There is a higher chance of collision or more number of collisions when you cramp up the space among the molecules.Hence, the rate of a reaction also increases on increasing the concentration of the reactants.