List of Laws for SAT II Chemistry?

Question

Does anyone know if there is a list of all the laws (like Pauli's Exclusion Principle, Law of Multiple Proportions, etc) online somewhere that could be on the subject test? I don't want to go through my entire review to make it a list if there are already some lists available.

Answer 1

here are some practice questions and answers

1. Ice, unlike most substances, is denser than water in the liquid phase.    BECAUSE    In water, hydrogen bonds can form between the positively charged H atom on one water molecule and the slightly negatively charged O atom on a nearby water molecule.

  

2.  Which of the following gases would be the densest at standard temperature and pressure?  

(A) Helium  

(B) Argon

(C) Carbon dioxide

(D) Xenon

(E) Nitrogen

  

3.  In the laboratory, a sample of hydrogen is collected by water displacement. The sample of hydrogen has a volume of 25 mL at 24.0ºC and a barometric pressure for the day of 758 mmHg. What is the pressure of the dry gas at this temperature? (The vapor pressure of water at 24.0ºC is 22.4 mmHg.)

(A) 455 mmHg

(B) 470 mmHg

(C) 736 mmHg

(D) 758 mmHg

(E) 780 mmHg

  

4.  Calculate the approximate amount of heat necessary to raise the temperature of 50.0 grams of liquid water from 10.0ºC to 30.0ºC. (The specific heat of water liquid is 4.18 J/gºC.)

(A) 20 J

(B) 80 J

(C) 100 J

(D) 200 J

(E) 4,180 J

  

5.  Using the sketch of the phase diagram for water given above, determine which of the following statements is incorrect:

(A) The triple point is point A. This is the point at which all three phases are in equilibrium with one another.

(B) The line AB is the line representing the solid-liquid equilibrium line. Anywhere along this line the substance could melt or freeze.

(C) The slope of line AB is negative. This slope indicates that the solid is much denser than the liquid.  

(D) Line AD represents the phase changes of sublimation and deposition.

(E) Line AC represents where the substance would condense and vaporize.



Statement I  Statement II

6. Most ionic solids have high melting points.   BECAUSE    Ionic solids are made up of positive and negative ions held together by electrostatic attractions.

  

7.  Which of the following best illustrates a graph of pressure versus volume for a gas at constant temperature?  

(A)  

(B)  

(C)  

(D)  

(E)  

  

8.  Which of the following solutions would probably have the highest boiling point?

(A) 0.100 m KOH

(B) 0.100 m Na2SO4

(C) 0.100 m C6H12O6

(D) 0.200 m CaCl2

(E) 0.200 m CH3CH2OH

  

9.  Which of the following must be measured in order to calculate the molality of a solution?

   I. Mass of the solute

II. Mass of the solvent

III. Total volume of the solution



(A) I only

(B) I and III only

(C) II and III only

(D) I and II only

(E) I, II, and III



  

10.  The molarity of a solution that is composed of 80.00 g of sodium hydroxide dissolved in 2.0 L of solution is

(A) 1.0 M

(B) 2.0 M  

(C) 4.0 M  

(D) 40.0 M  

(E) 160.0 M  

  

11.  Which of the following substances would dissociate completely when placed into excess amounts of distilled water?

(A) C2H5OH

(B) HC2H3O2

(C) LiNO3

(D) Mg(OH)2

(E) All of these will dissociate completely in water



Statement I  Statement II

12. The solubility of carbon dioxide in a soft drink decreases with a decrease in pressure.    BECAUSE    The solubility of a gas generally increases with an increase in temperature.  

  

13.  The molarity of a solution obtained when 50.0 mL of 6.0 M HCl is diluted to a final volume of 300.0 mL is

(A) 0.01 M

(B) 0.10 M

(C) 0.20 M

(D) 0.30 M

(E) 1.0 M

  

14.  Which of the following solutes and solvents would be expected to form stable solutions?

  

(A) I only

(B) I and II only

(C) III only

(D) I, II, and III only

(E) I, II, and IV only

1.      F, T    

(Do not fill in CE.) The first statement is false—water is actually less dense in its solid, frozen form, which is not true of most liquids. This is due to the hydrogen bonds that form between water molecules in water’s liquid state. When the temperature of water becomes low enough that water freezes, the molecules are locked into a regular, crystal lattice structure in which the molecules are actually farther apart from each other than they are when water is in its liquid state. The second statement is true, but since the first is false, there is no need to fill in the CE oval.

2.      D    

You’ll need to use the periodic table you’re given during the exam to answer this question since you’ll have to find the masses of the gases. Remember that the density of a gas is measured in grams per liter and that you will calculate the volume using the standard for gases at STP: 22.4 L per mole. Finally, remember that the heavier the molecule, the more dense the gas. A Helium is only 4 g/mol, B argon is 40 g/mol, C carbon dioxide is 44 g/mol, D xenon is 131 g/mol, and E nitrogen (N2) is diatomic, so this means it has a mass of 28 g/mol. The best choice is D, xenon.

3.      C    

This question appears to be very involved, so you might be tempted to use the ideal gas equation; however, the question only asks for the pressure of the dry gas. You’re given atmospheric pressure and water vapor pressure at the defined temperature, so all you need to do is subtract the water vapor from the atmospheric pressure: 758 mmHg - 22.4 mmHg = 735.6 mmHg; this matches C. Since you will not have a calculator, round numbers off: 760 - 20 = 740. The closest answer choice is C.

4.      E    

In this problem, the phase does not change; liquid water increases in temperature by 20.0˚C. This will take energy—to calculate the energy, use the equation q = mCp DT. You have all the information that you need: Q = (50.0 g)(4.184 J/gºC) (20.0ºC). Again, make the math easy: approximate that 2050 = 1000, then multiply by 4 to get 4000 J—the only answer choice that’s close is choice E.

5.      C    

A is the triple point, so this statement is true. B is the line that separates the solid and the liquid, so this is also a true statement. C is the answer. The slope of this line is not negative; it is positive. The second half of the statement is true: when there is a positive slope, the solid is more dense than the liquid. D is where the solid and vapor phase meet, so this statement is also true—sublimation and deposition are the changes of state associated with solids and gases. Finally, E is also a true statement—the line represents where the liquid meets the vapor, and so these changes of state could take place.

6.      T, T    

(Fill in CE.) The first statement is true: most ionic solids are characterized as having a high melting point. Ionic solids are also hard and brittle, with poor thermal and electrical conduction. The second statement is also true—ionic solids consist of positive and negative ions held together by electrostatic attractions, and you should fill in CE because the second statement is the reason for the first statement’s being true.

7.      E    

To answer this question, you must think about the relationship between pressure and volume. Boyle’s law states that if the pressure is increased, the volume will decrease if all other factors are held constant. This type of relationship is an inverse relationship, and choice E is the only graph that shows an inverse relationship.

8.      D    

The boiling point of a solution depends on the solution’s concentration in molality and the number of ions that exist in solution. First eliminate any answer choices that contain organic compounds, since carbon compounds are covalently bonded and do not disassociate into ions in solution; in this way you can eliminates choices C and E. Choice A would produce two ions in solution, choice B would produce three ions in solution, and choice D would produce three ions in solution. Now you must choose between B and D. Since the molality is greater in D and D produces the same number of ions, it would have the highest boiling point.

9.      D    

This question requires that you know the definition of molality: molality is the number of moles of solute per kilogram of solvent. Since moles are not directly measured, instead the mass of the solute, (I), would be the component measured in the laboratory. The mass of the solvent can be expressed in kilograms of solvent, or (II). The total volume, (III), is not needed to calculate molality—just molarity, so look for an answer that contains both (I) and (II); the answer is D.

10.      A    

This question asks you to calculate the molarity, which is the moles of solute per liter of solution. 80.0 grams of NaOH can be converted to moles by dividing 80 by 40 (the molecular weight of NaOH), and this gives you 2 moles. Now divide 2 by 2 to get 1.0 M, which is answer choice A.

11.      C    

This question in essence asks which of the answer choices is a strong electrolyte. Strong electrolytes are strong acids, strong bases, and soluble salts. Let’s go through the answer choices. Choice A is not a strong electrolyte—it’s an alcohol. Choice B is acetic acid, an organic acid, and is only a weak electrolyte. Choice C is a soluble salt; all nitrates are soluble and thus dissociate in solution. This is the correct answer. Choice D is ionically bonded but is not a strong base. In group 2A, only barium, strontium, and calcium hydroxides are considered to be strong. Mg(OH)2 is a chalky white liquid often taken as a laxative.

12.      T, F      

(Do not fill in CE.) Statement I is true—when the pressure of a system is decreased, the solubility of a gas decreases; as you probably know from experience, when you open a soda bottle, the pressure of the system decreases significantly, and gas bubbles rise to the top and escape. Statement II says that heating a gas in a solution will make the gas more soluble; this is not true. Since this statement is false, you would not fill in the CE oval.

13.      E    

This is a dilution problem, so use the formula you learned in this chapter to solv