Akins Chemistry Final

What is....The temperature and pressure at which the gas and liquid states of a substance become identical and form one phase?

Critical Point

What is....The temperature at which a substance changes from liquid to a gas at standard atmospheric pressure?

Normal Boiling Point

What is....The temperature and pressure conditions at which the solid, liquid, and gaseous phases of a substance coexist at equilibrium?

Triple Point

What is....The partial pressure exerted by a vapor that is in equilibrium with its liquid state at a given temperature?

Vapor Pressure

Standard temperature and pressure for a gas is a. 0°C and 1 atm. b. 0 K and 1 atm. c. 0°C and 1 Pa. d. 0 K and 1 Pa.

a. 0°C and 1 atm.

What is the concentration of OH- in pure water? a. 1.00 ´ 10-7 M b. 0.7 M c. 55.4 M d. 1.00 ´ 107 M

a. 1.00 ´ 10-7 M

What is the pH of a 1 ´ 10-4 M HCl solution? a. 4 b. 6 c. 8 d. 10

a. 4

A dissolved solute that does not form ions is a. a nonelectrolyte. b. a weak electrolyte. c. a strong electrolyte. d. insoluble.

a. a nonelectrolyte.

The actual yield of a chemical reaction is Select one: a. less than the theoretical yield. b. greater than the theoretical yield. c. equal to the percentage yield. d. greater than the percentage yield.

a. less than the theoretical yield.

If one knows the mass and molar mass of reactant A and the molar mass of product D in a chemical reaction, one can determine the mass of product D produced by using the a. mole ratio of D to A from the chemical equation. b. group numbers of the elements of A and D in the periodic table. c. estimating bond energies involved in the reaction. d. electron configurations of the atoms in A and D.

a. mole ratio of D to A from the chemical equation.

Which of the following is soluble in water? a. potassium nitrate b. silver c. benzene d. carbon tetrachloride

a. potassium nitrate

Which of the following is an electrolyte? a. sodium chloride b. sugar c. water d. glass

a. sodium chloride

What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L of solution? a. 0.0132 M b. 0.0253 M c. 0.459 M d. 1.363 M

b. 0.0253 M Molarity= moles of solute/liters of solution

Dissolved in water to make 100 mL of solution, 1.00 g of NaCl would have a concentration of a. 1.71 M. b. 0.171 M. c. 0.0171 M. d. 17.1 M.

b. 0.171 M. Molarity= moles of solute/liters of solution

What is the value of the self-ionization constant of water? a. 0 b. 1.00 ´ 10-14 c. 1.00 ´ 10-7 d. 55.4

b. 1.00 ´ 10-14

In the reaction N2 + 3H2 ® 2NH3, what is the mole ratio of nitrogen to ammonia? a. 1:1 b. 1:2 c. 1:3 d. 2:3

b. 1:2

What happens to the volume of a gas during compression? a. The volume increases. b. The volume decreases. c. The volume remains constant. d. It is impossible to tell because all gases are different.

b. The volume decreases.

Which of the following best describes temperature? a. heat absorbed or released in a chemical or physical change b. a measure of the average kinetic energy of the particles in a sample of matter c. heat energy d. energy of change

b. a measure of the average kinetic energy of the particles in a sample of matter

A solid with a low melting point is most likely a. ionic. b. covalent. c. metallic. d. None of the above

b. covalent.

A hydrogen bond is a special form of a(n) a. covalent bond. b. dipole-dipole force. c. ionic bond. d. London dispersion force.

b. dipole-dipole force.

A water solution whose pH is 10 a. is always neutral. b. is always basic. c. is always acidic. d. might be neutral, basic or acidic.

b. is always basic.

A chemical reaction involving substances A and B stops when B is completely used. B is the a. excess reactant. b. limiting reactant. c. primary reactant. d. primary product.

b. limiting reactant.

What is the SI unit of pressure? a. torr b. pascal c. pound d. newton

b. pascal

For the reaction represented by the equation 2H2 + O2® 2H2O, how many moles of water can be produced from 6.0 mol of oxygen? a. 2.0 mol b. 6.0 mol c. 12 mol d. 18 mol

c. 12 mol

What is the mole ratio of oxygen to phosphorus(V) oxide in the reaction P4(s) + 5O2(g) ® P4O10(s)? Select one: a. 1:1 b. 1:5 c. 5:1 d. 4:10

c. 5:1

For the reaction represented by the equation AgNO3 + NaCl ® NaNO3 + AgCl, how many moles of silver chloride, AgCl, are produced from 7.0 mol of silver nitrate AgNO3? a. 1.0 mol b. 2.3 mol c. 7.0 mol d. 21 mol

c. 7.0 mol

A sample of a gas occupies a volume of 752 mL at 25°C. What volume will the gas occupies if the temperature increases to 50°C, if the pressure remains constant? a. 376 mL b. 694 mL c. 815 mL d. 1500 mL

c. 815 mL Charles Law V₁/T₁=V₂/T₂ Temperature in Kelvin K=C+273

The solubility of a substance at a given temperature can be expressed as a. grams of solute. b. grams of solvent. c. amount of solute per amount of solvent. d. grams of water per 100 g of solute.

c. amount of solute per amount of solvent.

The strength of the forces between ions depends on a. the size of the ion only. b. the charge on the ion only. c. both the size of the ion and its charge. d. neither the size of the ion nor its charge.

c. both the size of the ion and its charge.

Which of the following has a melting point greater than room temperature? a. oxygen b. water c. iron d. bromine

c. iron

A very low value of the equilibrium constant for a reaction can indicate that a. equilibrium is reached slowly. b. products are favored. c. reactants are favored. d. equilibrium has been reached.

c. reactants are favored.

The kinetic-molecular theory states that gas particles are very far apart. This idea explains _____ of a gas. a. the fluidity b. the compressibility c. the fluidity and compressibility d. neither the fluidity nor the compressibility

c. the fluidity and compressibility

In the reaction Ca + Cl2 ® CaCl2, what is the mole ratio of chlorine to calcium chloride? a. 2:3 b. 2:1 c. 1:2 d. 1:1

d. 1:1

An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume? a. 0.623 L b. 0.911 L c. 1.05 L d. 3.42 L

d. 3.42 L Volume= moles of solute/Molarity

For the reaction SO3 + H2O ® H2SO4, calculate the percentage yield if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid. a. 82.7% b. 88.3% c. 91.2% d. 93.9%

d. 93.9% Percent yield=actual yield/theoretical yield x 100

Which of the following expresses concentration? a. molality b. molarity c. parts per million d. All of the above

d. All of the above

Which is not an assumption of the kinetic-molecular theory? a. Matter is composed of tiny particles. b. The particles of matter are in continual motion. c. The particles of a gas are far relatively apart. d. When individual gas particles collide, the collision is inelastic.

d. When individual gas particles collide, the collision is inelastic.

What is the measured amount of a product obtained from a chemical reaction? a. mole ratio b. percentage yield c. theoretical yield d. actual yield

d. actual yield

A London dispersion force is considered a dipole-dipole force because it a. affects all types of compounds. b. affects nonpolar molecules. c. affects polar molecules. d. results from a temporary dipole.

d. results from a temporary dipole.

In a solution at equilibrium, a. no dissolution occurs. b. the rate of dissolution is less than the rate of crystallization. c. the rate of dissolution is greater than the rate of crystallization. d. the rate of dissolution and the rate of crystallization are equal.

d. the rate of dissolution and the rate of crystallization are equal.