At given concentrations of A and B, molecules of A and B collide to produce AB at a particular rate. If the concentration of B is increased, then molecules of A collide with molecules of B frequently because more molecules of B are available. More collisions ultimately the rate of reaction.

As the temperature of a chemical reaction increases, the rate of reaction increases becauseA fewer particle collisions occurB the required activation energy increasesC more effective particle collisions occurD the concentration of the reactants increases

Why does decreasing the concentration of the reactants generally result in a lower reaction rate?Question 4Select one:a.There are more collisions between reactant molecules.b.The reactant molecules collide with greater energy.c.The reactant molecules collide with less energy.d.There are fewer collisions between reactant molecules.

you studied the effect of concentration on the rate of reaction. Explain your observations using the collision theory

How are the rates of chemical reactions related to collisions between reacting particles?Multiple select question.Reacting substances must collide at slow enough speeds for energy transfer to occur.Reacting substances must collide in the correct orientation.Reacting substances (atoms, ions, or molecules) must collide.Reacting substances must collide with sufficient energy to form an activated complex.

For the same mass, many small pieces have more total than one large chunk. Therefore, the collision rate between reacting particles increases and the rate of reaction .