Kinetics

Question 1

Kinetics

Answer 1

deals with the rates of chemical reactions

Question 2

rate

Answer 2

describes how fast a reaction takes place

Question 3

Effective Collision Theory

Answer 3

for reactions to occur reactant particles must collide
1. spatial orientation must be exact
2. activation energy must be met

Question 4

What causes more effective reaction rates?

Answer 4

an increase in temp due to more KE, and a greater amount of concentration of reactants, ionic substances react faster than covalent because covalent are larger and contain more bonds, increase in surface area because more of the surface is exposed, pressure bc it increases the concentration of the particles, and if there is a catalyst it increases the reaction rate by lowering the activation energy and creating an alternative path

Question 5

Potential Energy

Answer 5

is the energy stored within the bonds of reactants and products of a reaction

Question 6

Heat Constant (heat of reaction)

Answer 6

amount of heat absorbed or released in a chemical reaction (PE of the products - PE of the reactants )

Question 7

Endothermic Reactions

Answer 7

gain more energy than is released, energy of the products is higher than the reactants; delta H is always +

Question 8

Exothermic Reactions

Answer 8

more energy is lost to the surroundings; products have less energy than the reactants; energy was released; delta h is negative

Question 9

Delta H

Answer 9

difference between the energy needed to break the bonds in the reactants, and the energy given out when new bonds are formed in the products

Question 10

Heat of Reaction

Answer 10

difference in PE of the products and the PE of the reactants

Question 11

Exothermic Reactions - Surrounding Temps

Answer 11

release energy so the surrounding temperature gets warmer

Question 12

Endothermic Reactions - Surrounding Temps

Answer 12

absorb energy so the surrounding temperature gets colder