1. Reversible Reaction- A reaction in which products can be changed back to reactants by reversing the conditions.

2. Equilibrium (reaction)- A reaction that does not go to completion and in which reactants and products are present in fixed concentration ratios.

3. 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.

4. Closed system- A system in which matter or energy is not lost or gained, e.g. gases in a closed vessel.

5. Open system- A system in which matter is lost or gained, e.g. a mixture of solids and gases in an open beaker

6. Le Chatelier’s Principle- When any of the conditions affecting the position of equilibrium are changed, the position of that equilibrium shifts to minimize the change.

7. Equilibrium Constant (K[subscript c])- a constant calculated from the equilibrium expression for a reaction.

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

9. 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)).

10. Partial Pressure- the pressure that an individual gas contributes to the overall pressure in a mixture of gases.

11. Acid- A proton (hydrogen ion) donor.

12. Base- A proton (hydrogen ion) acceptor.

13. alkali- A base that is soluble in water.

14. Brønsted-Lowry Acid- A proton Donor.

15. Brønsted-Lowry Base- A proton Acceptor.

16. Amphoteric- Able to behave as both an acid and a base, e.g. aluminum oxide.

17. Arrhenius Acid- Any species that increases the concentration of H^+ in an aqueous solution.

18. Arrhenius Base- Any species that increases the concentration of OH^- in an aqueous solution.

19. Brønsted-Lowry Theory (of acids and bases)- Acids are proton donors and bases are proton acceptors.

20. 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. the acid in the forward reaction and the base in the reverse reaction or the base in the forward reaction and the acid in the reverse reaction.

21. 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.

22. Strong Acid/Base- An acid or base that is (almost) completely ionized in water.

23. Weak Acid/Base- An acid or base that is only slightly ionized in water.

    (Chapter 13 Begins)

24. Eutrophication- An environmental problem caused by fertilizers leached from fields into rivers and lakes. The fertilizer then promotes the growth of algae on the surface of the water. When the algae die, bacteria thrive and use up the dissolved oxygen in the water, killing aquatic life.

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

26. Contact Process- Synthesis of Sulfuric Acid. Involves three equations irl but two for us rn:

    1. 2SO2(g) + O2(g) ⇌ 2SO3(g) ΔHr= -197 KJ/mol

    2. SO3(g) + H2O(l) → H2SO4(aq)

   Fun Fact: the actual contact process goes like this:

   a. Contact Tower: 2SO2(g) + O2(g) ⇌ 2SO3(g) ΔHr= -197 KJ/mo; V2O5 catalyst and 450\*C

   b. Absorption Tower: SO3(g) + H2SO4(aq)→ H2S2O7(aq) (oleum)

   c. Dilution Tower: H2S2O7(aq) + H2O(l)→ 2H2SO4(aq)

   (This factors in the fact that the products can react with the reactants sometimes)