Stm 006 Module 17-18

Front 1

is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.

Back 1

Reversible Reaction

Front 2

will reach an equilibrium point where the concentrations of the reactants and products will no longer change.

Back 2

Reversible Reactions

Front 3

is denoted by a double arrow pointing both directions in a chemical equation

Back 3

Reversible Reaction

Front 4

Some chemical reactions can occur in only one direction. These reactions are called

Back 4

irreversible reactions

Front 5

The reactants can change to the products, but the products cannot change back to the reactants.

Back 5

Irreversible reactions

Front 6

French chemist? introduced the concept of reversible reactions

Back 6

Claude Louis Berthollet

Front 7

he observed that sodium carbonate and calcium chloride react to yield calcium carbonate and sodium chloride

Back 7

Claude Louis Berthollet

Front 8

These equations typically have a unidirectional arrow (—>—>) to represent irreversible reactions. Other chemical equations may have a bidirectional harpoons (arrow alternate) that represent reversible reactions

Back 8

Important

Front 9

A fundamental concept of chemistry is that chemical reactions occurred when reactants reacted with each other to form products.

Back 9

Irreversible Reactions

Front 10

These unidirectional reactions are known as?, reactions in which the reactants convert to products and where the producis cannot convert back to the reactants

Back 10

irreversible reactions

Front 11

- An example of an is combustion. Combustion involves burning an organic compound

Back 11

irreversible reaction

Front 12

The reactants and products are never fully consumed; they are each constantly reacting and being produced

Back 12

reversible reactions

Front 13

When the reactants and products of a reaction are mixed, it is hard to tell if the system is at equilibrium

Back 13

reactions quotient

Front 14

What we can do is calculate a reaction quotient using the same formula as the equilibrium constant.

Back 14

Reactions quotient

Front 15

depending on the size of the reaction quotient, we can compare it to the known value of the equilibrium constant to determine the direction the reaction is moving

Back 15

Important

Front 16

What kind of reaction happens when the reactants and products are never fully consumed

Back 16

Reversible reaction