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Question 1

K_eq

Answer 1

Equilibrium Constant

Question 2

Equilibrium Expression

Answer 2

Product of Products (raised to coefficient powers)

OVER

Product of Reactants (raised to coefficient powers)

Question 3

Given: reaction is at equilibrium

Given: K_eq > 1

Which side is favored: products or reactants?

Answer 3

PRODUCTS

If K > 1, Products are greater percentage of system

(If K < 1, Reactants are greater percentage of system)

Question 4

R

I

C

E

Answer 4

Reaction

Initial concentrations

Change in concentrations

Equilibrium concentrations

Question 5

If Q = K_eq

Answer 5

Reaction is at equilibrium

Question 6

If Q > K_eq

Answer 6

Reaction is NOT at equilibrium

Reaction will proceed towards equilibrium by shifting Left

(If Q is BIG, products are big. Products are STRESSED.)

Question 7

If Q < K_eq

Answer 7

Reaction is NOT at equilibrium

Reaction will proceed towards equilibrium by shifting RIGHT

(If Q is small, products are small. Reactants are STRESSED.)

Question 8

Law of Mass Action

Answer 8

Question 9

ICE equations

Answer 9

I plus C equals E

Question 10

LeChatelier’s Principle

Answer 10

A change in conditions will STRESS one side of reaction.

Equilibrium will shift in to OTHER side.

Question 11

What species are NOT included in equilibrium expression (K_eq equation)?

Answer 11

Pure solids and pure liquids

Question 12

First step in solving ICE problem

Answer 12

Balance chemical reaction!

Question 13

Second step in solving RICE/ICE problem

Answer 13

Fill out RICE table

Figure out knowns and unknowns, including K_eq

Question 14

Third step in solving RICE/ICE problems

Answer 14

Write down equations (I+C=E & K_eq)

Confirm # of knowns = # of unknowns

Solve for WHAT IS ASKED FOR!!

Question 15

NH₄Cl(s) ⇔ NH₃(g) + HCl(g)

An increase in NH₃(g) concentration put into the system STRESSES which side?

Answer 15

RIght (Products)

Question 16

NH₄Cl(s) ⇔ NH₃(g) + HCl(g)

An increase in pressure put into the system STRESSES which side?

Answer 16

The side with more pressure, which is the side with more moles of gas. The left side has zero moles of gas. The right side has 2 moles of gas.

Answer: Right (Products)

Question 17

NH₄Cl(s) ⇔ NH₃(g) + HCl(g)

An increase in NH₃(g) concentration put into the system will shift equilibrium to which side?

Answer 17

Left (Reactants)

The right side gets stressed, which shifts the equilibrium to the left.

Question 19

NH₄Cl(s) ⇔ NH₃(g) + HCl(g)

An increase in pressure put into the system shifts equilibrium to which side?

Answer 19

Increased pressure STRESSES the right side (the side with more moles of gas). This SHIFTS the equilibrium to favor the other side more, to relieve the pressure.

Answer: Left (Reactants)

Question 20

H₂(g)+ I₂(g)⇔ 2HI(g)+ heat

An increase in temperature (to the whole system) will STRESS which side?

Answer 20

Right (Products)

Question 21

H₂(g)+ I₂(g)⇔ 2HI(g)+ heat

An increase in temperature (to the whole system) will SHIFT equilibrium favor to which side?

Answer 21

Left (Reactants)

Question 22

Endothermic Reaction

Answer 22

Energy is absorbed by reactants

Write HEAT next to reactants

positive delta H

Question 23

Exothermic Reaction

Answer 23

Energy is released by products

Write HEAT next to products

negative delta H

Question 24

Haber Process

Answer 24

3H₂(g) + N₂(g) ⇔ NH₃(g) + heat

Fritz Haber

Germans used it to make explosives in WWI

Enabled HUGE increase in nitrogen fertilizer production which enabled HUGE increase in food production (growing crops) which enabled massive world population growth in 1900s

Question 26

In Keq expression what is the concentration of H20?

Answer 26

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