Jeopardy

1
Jeopardy
Solutions Kinetics Equilibrium Solubility and Qual Pot Pourri
100 100 100 100 100
200 200 200 200 200
300 300 300 300 300
400 400 400 400 400
500 500 500 500 500
2
100 Solutions

• What information do you need to determine the
  molality of a 5.0 M solution of sucrose?

3
200 Solutions

• A student wishes to prepare 0.50 liters of 0.8300
  molar KIO3 (molecular weight 214). The proper
  procedure is to weigh out_______________

4
300 Solutions

• What is the final concentration of barium ions,
  Ba2, in solution when 100. mL of 0.30 M
  BaCl2(aq) is mixed with 100. mL of 0.100 M
  H2SO4(aq)?
• .1M

5
400 Solutions

• How many milliliters of 15.8-molar NaOH must be
  diluted to obtain 2.5 liter of 4.0-molar NaOH?

6
500 Solutions

What is the minimal information needed to
determine the molar mass of a solute by freezing
point depression?
7
100 Kinetics

• What does a catalyst do to the rate of a
  reaction? Why? (Draw a graph showing this)
• Speeds it up, by lowering the activation energy

8
200 Kinetics

• The isomerization of cyclopropane to propylene is
  a first-order process with a half-life of 76
  minutes at 300?C. The time it takes for the
  partial pressure of cyclopropane to decrease from
  2.0 atmosphere to 0.5 atmosphere at 300?C is
  closest to
• 152 minutes

9
300 Kinetics

• H3AsO4 3 I- 2 H3O ?H3AsO3 I3- H2O
• The oxidation of iodide ions by arsenic acid in
  acidic aqueous solution occurs according to the
  stoichiometry shown above. The experimental rate
  law of the reaction is
• Rate kH3AsO4 I- H3O
• According to the rate law for the reaction, an
  increase in the concentration of Iodide ion has
  what effect on this reaction?

10
400 Kinetics

• 2 A(g) B(g) ? 2 C(g)
• When the concentration of substance B in the
  reaction above is doubled, all other factors
  being held constant, it is found that the rate of
  the reaction remains unchanged. Explain this
  observation in terms of the reaction mechanism.

11
500 Kinetics

• (CH3)3CCl(aq) OH- ? (CH3)3COH(aq) Cl-
• For the reaction represented above, the
  experimental rate law is given as follows.
• Rate k(CH3)3CCl
• If some solid sodium solid hydroxide is added to
  a solution that is 0.010 molar in (CH3)3CCl and
  0.10 molar in NaOH, What will happen to the rate
  and k?

12
100 Equilibrium

• CuO(s) H2(g) ? Cu(s) H2O(g)
• ?H -2.0 kilojoules
• When the substances in the equation above are at
  equilibrium at pressure P and temperature T, how
  can you shift the equilibrium to favor the
  reactants?

13
200 Equilibrium

• If 2.5 mol of N2O4 gas is reacted in a 7.0 L
  container, what is the equilibrium concentration
  of NO2 in the container?
• K 4.0 x 10-7

14
300 Equilibrium

• PCl3(g) Cl2(g) ? PCl5(g) energy
• Some PCl3 and Cl2 are mixed in a container at
  200?C and the system reaches equilibrium
  according to the equation above. Which of the
  following causes an increase in the number of
  moles of PCl5 present at equilibrium?
• I. Decreasing the volume of the container
• II. Raising the temperature
• III. Adding a mole of He gas at constant volume

15
400 Equilibrium
SO2(g) O2(g) ?2 SO3(g) When 0.40 mole of SO2
and 0.60 mole of O2 are placed in an evacuated
1.00 liter flask, the reaction represented above
occurs. After the reactants and the product reach
equilibrium and the initial temperature is
restored, the flask is found to contain 0.30 mole
of SO3. Based on these results, the equilibrium
constant, Kc, for the reaction is
16
500 Equilibrium

• In which of the following systems would the
  number of moles of the substances present at
  equilibrium NOT be shifted by a change in the
  volume of the system at constant temperature?
• a. CO(g) NO(g) ? CO2(g) 1/2 N2(g)
• b. N2(g) 3 H2(g) ? 2 NH3(g)
• c. N2(g) 2 O2(g) ? 2 NO2(g)
• d. N2O4(g) ? 2 NO2(g)
• e. NO(g) O3(g) ? NO2(g) O2(g)

17
100 Solubility Qual

• How many moles of NaF must be dissolved in 1.00
  liter of a saturated solution of PbF2 at 25ºC to
  reduce the Pb2 to 1x10-6 molar? (Ksp PbF2 at
  25 ºC 4.0x10-8)

18
200 Solubility Qual

• Barium sulfate is LEAST soluble in a 0.01 molar
  solution of which of the following?
• a. Al2(SO4)3 d. NH3
• b. (NH4)2SO4 e. BaCl2
• c. Na2SO4

19
300 Solubility Qual

• When dilute nitric acid was added to a solution
  of one of the following chemicals, a gas was
  evolved. This gas turned a drop of limewater,
  Ca(OH)2, cloudy, due to the formation of a white
  precipitate. The chemical contained which of the
  following ions? (Sodium, bicarbonate, Magnesium,
  Ammonium, Sulfate)

20
400 Solubility Qual

• A 20.0 milliliter sample of 0.200 molar K2CO3
  solution is added to 30.0 milliliters of 0.400
  molar Ba(NO3)2 solution. Barium carbonate
  precipitates. The concentration of barium ion,
  Ba2, in solution after reaction is

21
500 Solubility Qual

• What is the equilibrium concentration of chloride
  ions when 100 mL of .4 M AgNO3 is mixed with 200
  mL of .4M NaCl?

22
100 Pot Pourri

• What is an electrolyte?

23
200 Pot Pourri

• A solution of 1.0 M NaCl is diluted. What
  happens to volume, moles, and molarity of NaCl?

24
300 Pot Pourri

• Rank the following three substances from weakest
  to strongest electrolyte.
• HNO3
• C12H22O11
• HC2H3O2

25
400 Pot Pourri

• Consider the reaction K4.85
• 200. g of NH4NO3(s) are placed in a reaction
  vessel containing H2O(g) at a concentration of
  2.0 M and N2O(g) at a concentration of 2.0 M.
  After equilibrium is reached, will the mass of
  NH4NO3(s) increase, decrease or remain unchanged?
  

26
500 Pot Pourri

• What is the mole fraction of ethanol, C2H5OH, in
  an aqueous solution in which the ethanol
  concentration is 4.6 molal?