Chapter 8 and 13 Vocabulary

Reversible Reaction

A reaction in which products can be changed back to reactants by reversing the conditions

Equilibrium (reaction)

A reaction that does not go to completion and in which reactants and products are present in fixed concentration ratios

Dynamic (Equilibrium)

In an equilibrium mixture, the molecules of reactants are being converted to products at the same rate as products are being converted to reactants

Closed system

A system in which matter or energy is not lost or gained, e.g

Open system

A system in which matter is lost or gained, e.g

Le Chateliers Principle

When any of the conditions affecting the position of equilibrium are changed, the position of that equilibrium shifts to minimize the change

Equilibrium Constant (K[subscript c])

a constant calculated from the equilibrium expression for a reaction

Equilibrium Expression

A simple relationship that links K[subscript c] to the equilibrium concentrations of reactants and products and the stoichiometric equation

Reaction Quotient

A measure of the relative amounts of products and reactants present in a reaction at a given time, Q=(([C]^c)([D]^d))/(([A]^a)([B]^b))

Partial Pressure

the pressure that an individual gas contributes to the overall pressure in a mixture of gases

Acid

A proton (hydrogen ion) donor

Base

A proton (hydrogen ion) acceptor

alkali

A base that is soluble in water

Brønsted-Lowry Acid

A proton Donor

Brønsted-Lowry Base

A proton Acceptor

Amphoteric

Able to behave as both an acid and a base, e.g

Arrhenius Acid

Any species that increases the concentration of H^+ in an aqueous solution

Brønsted-Lowry Theory (of acids and bases)

Acids are proton donors and bases are proton acceptors

Conjugate Pair (acid/base)

An acid and base on each side of an equilibrium equation that are related to each other by the difference of a proton; e.g

Strong Acid/Base

An acid or base that is (almost) completely ionized in water

Weak Acid/Base

An acid or base that is only slightly ionized in water

Eutrophication

An environmental problem caused by fertilizers leached from fields into rivers and lakes

Haber Process

Synthesis of ammonia, N2(g) + H2(g)⇌ 2NH3(g) ΔHr= -92 KJ/mol, Fe catalyst drawn above yield arrows

Contact Process

Synthesis of Sulfuric Acid

Arrhenius Base

Any species that increases the concentration of OH^- in an aqueous solution

Dissociation

The break-up of a molecule :( into ions, for example, when HCl molecules dissolve in aqueous solution, they dissociate completely into H^+ and Cl^- ions.