Chemistry: Final Exam Review

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The decrease in concentration of reactants or the increase in concentration of products with time.

Increasing temperature causes the kinetic energy to increase. Thus, molecules are moving faster and colliding more frequently. This causes the rate of reaction to incrase.

Decreasing concentration leads to less reactants available for collision. Therefore, reaction rate decreases.

By increasing the surface area of reactant molecules, we are increasing the space or point of contact that these molecules have available to interact. This causes an increase in the rate of reaction.

A catalyst speeds up a chemical reaction by finding an alternate pathway with a lower activation energy.

The energy required to start a chemical reaction.

Equilibrium is established when the rate of the forward reaction is equal to the rate of the reverse reaction.

Absorbed.

Exothermic reactions release energy. The sign of delta H is negative.

Exothermic; heat is being given off.

The amount of heat required to raise 1g of a substance to 1 degrees Celsius.

Heat (kJ)

Specific heat capacity (J / g degrees C)

An acid.

A base.

Base.

Acid.

Base.

Acid

Base

When an acid reacts with a base to form water and a salt. pH = 7.

Base (tastes bitter)

Base (drain cleaners are bases).

Acid (tastes sour)

The part of the solution in less amount.

The part of the solution in greater amount. (HINT: solvent is a bigger word than solute)

1 mole = 6.02 x 10^23 atoms/molecules

1 mole of gas at STP = 22.4 L

Pressure = 1 atm or 101.3 kPa
Temperature = 0 degrees Celsius or 273 K

0 K (all molecular motion stops)

Gas molecules are constant motion and collide with the walls of their containers and with the surfaces that they come into contact with. This collision causes pressure.

Moles.

(Kelvin = Celsius + 273)
Answer: 298K

(Celsius = Kelvin - 273)
Answer: -175 degrees Celsius

4
He
2

0
B
-1

3.3 g H2

141.4 g CO2

2 H2 + O2 ----> 2 H20

1 C3H8 + 3 O2 ---> 5 CO2 + 4 H2O

342 g/mol

Gases

H - nonmetal
C - nonmetal
K - metal
Fe - transition metal
Si - semimetal

NO! They have a full octet of electrons. They do not want to react with anything.

Increasing temperature means heat is being added more to the left side (think mud slide). The reaction will shift right to form more NO.

Endothermic (going from solid --> liquid). Think about phase change diagram.

Going from gas ---> liquid. This is exothermic.

Going from liquid ---> gas. This is endothermic.

Going from liquid ---> solid. This is exothermic.

..
: Ne :
..

.
. C .
.

.
: F :
..

Weak acids dissociate partially. Strong acids and bases dissociate (break apart) completely in water.

C6H12O6 is a sugar that is covalently bonded. It does not conduct electricity.

NaCl is a salt and an electrolyte (conducts electricity).
NaOH is a strong base and therefore, strong electrolyte.
HCl is a strong acid and strong electrolyte.

*All salts, acids, and bases will conduct electricity.

Amino acids are the monomers.