Chemistry MC: October 2017

A) this compound should be called trisodium monophosphate.
B) the sodium has a negative 3 charge.
C) you cannot use a prefix for the first element in a molecular compound.
D) you cannot use a prefix for the first element of an ionic compound.
E) none of the above

Answer: D

Choose the pair of names and formulas that do NOT match.

A) copper(I) nitrate: CuNO3
B) copper(II) nitride: Cu3N2
C) copper(II) nitrate: Cu(NO3)2
D) copper(II) nitrite: Cu(NO2)2
E) all of these are correct

Answer: E

What is the correct name for the BrO41- ion?

A) hypobromite
B) perbromate
C) bromite
D) bromate
E) none of the above

Answer: B

What is the correct formula for the hypochlorite polyatomic ion?

A) ClO
B)ClO2-
C) ClO3-
D) ClO4-
E) none of the above

Answer: A

The charge of a vanadium ion in the compound V2O5 is:

A) 5+
B) 2+
C) 10+
D) 10-
E) none of the above

Answer: A

The formula for potassium chlorate is KClO3. The formula for magnesium chloride is MgCl2. What is the formula for magnesium chlorate?

A) MgClO3
B) Mg2ClO3
C) Mg(ClO3)2
D) Mg2(ClO3)3
E) none of the above

Answer: C

What is the correct formula for ammonium hydrogen sulfate?

A) NH4HSO4
B) (NH4)2HSO4
C) (NH4)2SO4
D) Am2HSO4
E) none of the above

Answer: A

What is the correct formula for potassium dichromate?

A) K(CrO4)2
B) KCr2O7
C) K2CrO4
D) K2Cr2O7
E) none of the above

Answer: D

What is the formula for the acetate polyatomic ion?

A) C3H2O3-
B) C2H3O22-
C) C2H3O2-
D) C2H3O
E)none of the above

Answer: C

What is the name of the compound whose formula is Na2O?

A) sodium monoxide
B) disodium oxide
C) disodium monoxide
D) sodium oxide
E) none of the above

Answer: D

Which formula shown is incorrect for the name given?

A) strontium carbonate: SrCO3
B) ammonium cyanide: NH4CN
C) potassium acetate: KC2H3O2
D) calcium nitrate: Ca(NO3)2
E) lithium sulfate: LiSO4

Answer: E

Which formula shown is incorrect for the name given?

A) magnesium nitrite: Mg(NO2)3
B) calcium carbonate: CaCO3
C) aluminum sulfate: Al2(SO4)3
D) sodium hydrogen carbonate: NaHCO3
E) potassium hydroxide: KOH

Answer: A

What is the name of Ca(NO3)2?

A) calcium dinitrite
B) calcium nitrate
C) calcium nitride
D) calcium nitrite
E) none of the above

Answer: B

What is the name of CoS?

A) cobalt(II) sulfide
B) cobalt sulfide
C) cobalt monosulfide
D) cobaltous sulfur
E) none of the above

Answer: A

Which metal atom below cannot form a cation of several different charges?

A) Cr
B) Mn
C) Fe
D) Ba
E) none of the above

Answer: D

What is the name of the compound made from lithium and oxygen?

A) lithium dioxide
B) lithium(I) oxide
C) oxygen lithide
D) lithium oxide
E) none of the above

Answer: D

What is the name of the ionic compound made of beryllium and chlorine?

A) beryllium(II) chloride
B) beryllium dichloride
C) beryllium chloride
D) monoberyllium dichloride
E) none of the above

Answer: C

A student wrote the formula for the compound aluminum phosphate as AlPO4 . What is wrong with this formula?

A) The compound is not charge-neutral.
B) Aluminum is a nonmetal so it cannot form an ionic compound.
C) The formula should be Al(PO4) .
D) There cannot be three different atom types in a chemical formula.
E) Nothing is wrong with the formula.

Answer: E

What is the formula for an ionic compound made of aluminum and oxygen?

A) AlO2
B) Al2O3
C) Al3O2
D) AlO
E) none of the above

Answer: B

The ionic compound that forms between potassium and oxygen is:

A) K2O.
B) KO.
C) KO2.
D) K2O2.
E) none of the above

Answer: A

What is the formula for an ionic compound made of carbon and oxygen?

A) CO2
B) C2O
C) CO
D) CO3
E) Carbon and oxygen do not form an ionic compound.

Answer: E

What is the formula for an ionic compound made of magnesium and sulfur?

A) MgS
B) MgS2
C) Mg2S
D) Mg2S3
E) none of the above

Answer: A

What is the formula for an ionic compound made of barium and nitrogen?

A) Ba3N2
B) Ba2N3
C) BaN
D) Ba2N4
E) none of the above

Answer: A

Which of the following is a molecular compound?

A) barium sulfide
B) calcium acetate
C) potassium hydroxide
D) nitrogen monoxide
E) none of the above

Answer: D

Which of the following species is a molecular element?

A) neon
B) sodium
C) chlorine
D) carbon dioxide
E) none of the above

Answer: C

Ammonium fluoride is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: D

Fluorine is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: B

Carbon monoxide is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: C

Which among the following elements does NOT exist as a diatomic molecule in nature?

A) hydrogen
B) nitrogen
C) fluorine
D) neon
E) none of the above

Answer: D

Carbon is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: A

What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms?

A) O10P4
B) 10OP4
C) 4PO10
D) P4O10
E) none of the above

Answer: D

What is the correct formula for a compound that has three oxygen atoms and one sulfur atom?

A) O3S
B) SO3
C) 3OS
D) SO3
E) none of the above

Answer: B

How many of each type of atom are there in the formula (NH4)2HPO4?

A) N = 2, H = 9, P = 1, O = 4
B) N = 1, H = 5, P = 1, O = 4
C) N = 2, H = 5, P = 1, O = 4
D) N = 2, H = 8, P = 1, O = 4
E) none of the above

Answer: A

How many of each type of atom are there in the formula Ca3(PO4)2?

A) Ca = 3, P = 1, O = 4
B) Ca = 3, P = 2, O = 4
C) Ca = 3, P = 2, O = 8
D) Ca = 3, P = 1, O = 8
E) none of the above

Answer: C

How many of each type of atoms are there in the formula NH4C2H3O2?

A) N = 4, H = 7, C = 2, O = 2
B) N = 1, H = 4, C = 2, O = 2
C) N = 1, H = 3, C = 2, O = 2
D) N = 1, H = 7, C = 2, O = 2
E) none of the above

Answer: D

Which formula shows the proper use of parentheses?

A) Ca(F)2
B) Ca(SO4)
C) (NH4)3(PO4)
D) Ca(NO3)2
E) none of the above

Answer: D

How many oxygen atoms are in the formula Al2(CO3)3?

A) 3
B) 9
C) 1
D) 6
E) none of the above

Answer: B

How many carbon atoms are in the formula Al2(CO3)3?

A) 3
B) 9
C) 1
D) 6
E) none of the above

Answer: A

How many total atoms are in the formula Al2(CO3)3?

A) 8
B) 9
C) 12
D) 14
E) none of the above

Answer: D

Which of the following statements about chemical formulas is FALSE?

A) The subscripts represent the relative number of each type of atom in the compound.
B) The subscripts represent the relative mass of each type of atom in the compound.
C) The subscripts do not change for a given compound.
D) Different compounds made of the same elements have different subscripts.
E) All of the statements are true.

Answer: B

Suppose an unknown compound XY has an X-to-Y mass ratio of 4.0. If decomposition of compound XY gives 12.0 grams of X, then how many grams of Y must form?

A) 48.0 grams
B) 12.0 grams
C) 4.0 grams
D) 3.0 grams
E) none of the above

Answer: D

What is the oxygen-to-sulfur mass ratio of sulfur dioxide?

A) 0.5
B) 1.0
C) 2.0
D) 16
E) none of the above

Answer: B

The phosphorous-to-hydrogen mass ratio is 10.2 for a compound. This ratio could correspond to the compound:

A) PH.
B) PH2.
C) PH3.
D) PH6.
E) none of the above

Answer: C

What is the oxygen-to-hydrogen mass ratio for H2O2?

A) 0.125
B) 4
C) 8
D) 16
E) none of the above

Answer: D

The oxygen-to-hydrogen mass ratio of water is always 8.0 is an example of what fundamental law?

A) Law of Constant Composition
B) Law of Constant Mass Ratio
C) Law of Conservation of Mass
D) Law of Constant Whole Number Ratio
E) none of the above

Answer: A

The law of constant composition states:

A) Matter cannot be either created or destroyed in a chemical reaction.
B) The nucleus is a dense region of positive charge that always contains protons and neutrons.
C) All samples of a given compound have the same proportions of their constituent elements.
D) All atoms of a given element have a constant composition and are different than atoms of any other element.
E) none of the above

Answer: C

The first chemist to formally state the law of constant composition was:

A) Dalton.
B) Mendeleev.
C) Rutherford.
D) Proust.
E) none of the above

Answer: D

When elements combine to form compounds:

A) their properties are an average of all elements in the compound.
B) their properties change completely.
C) their properties do not change.
D) their properties are completely random.
E) none of the above

Answer: B

If you put a living cell into seawater containing a higher concentration of sodium chloride, the cell loses water through osmosis.

Answer: TRUE

Osmosis is the process in which a solvent moves from an area of low solute concentration to an area of high solute concentration.

Answer: TRUE

A 0.10 molality solution of the sugar glucose (molecular weight = 180.10 g/mol) and a 0.10 molality solution of sucrose (molecular weight = 342.34 g/mol) would both boil at the same temperature.

Answer: TRUE

Upon completing a dilution from a stock solution, you will always have more volume of solution than you started with and it will have a lower concentration than the stock solution.

Answer: TRUE

A stock solution is a more concentrated form than what is typically used in a lab. It often requires further dilution.

Answer: TRUE

If 50 grams of salt dissolves into 250 grams of water, the resulting solution must have a mass of 300 grams.

Answer: TRUE

One liter of a 2.0 M NaOH (aq) solution contains the same number of Na+ ions as does one liter of a 1.0 M Na2CO3 (aq) solution.

Answer: TRUE

Molarity is defined as the moles of solute per liter of solution.

Answer: TRUE

A solution that is 13.58 percent by mass of sugar contains of sugar dissolved in of water.

Answer: TRUE

The solubility of gases in water increases with increasing pressure above the water.

Answer: TRUE

Warm beer goes flat quicker than cold beer.

Answer: TRUE

The solubility of gases in water decreases with increasing temperature.

Answer: TRUE

Tap water contains dissolved nitrogen and oxygen.

Answer: TRUE

The solubility of solids in water generally increases with increasing temperature.

Answer: TRUE

Salt water is an example of a strong electrolyte solution.

Answer: TRUE

A supersaturated solution is unstable and crystallization usually occurs.

Answer: TRUE

A saturated solution holds the maximum amount of solute under the solution conditions.

Answer: TRUE

It would be expected that methanol (CH3OH) would be more soluble in water than methane (CH4) would be.

Answer: TRUE

Vitamin C is a water-soluble vitamin, so it is likely that this vitamin is polar.

Answer: TRUE

The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.

Answer: TRUE

Steel is an example of a solid solution.

Answer: TRUE

Air is an example of a gaseous solution.

Answer: TRUE

A solution is a homogeneous mixture of two or more substances.

Answer: TRUE

Given that the freezing point depression constant for water is 1.86°C kg/mol, calculate the change in freezing point for a 0.907 M sugar solution.

A) 0.488°C
B) 2.05°C
C) 0.592°C
D) 1.69°C
E) none of the above

Answer: D

Calculate the molality of a solution prepared by dissolving 19.9 g of KCl in 750.0 ML of water.

A) 0.200
B) 0.356
C) 4.99
D) 0.267
E) none of the above

Answer: B

Determine the volume (liters) of 0.500M NaOH solution required to neutralize 1.50L of 0.750M H2SO4.

The neutralization reaction is

H2SO4 (aq) + 2NaOH (aq) ? Na2SO4 (aq) + 2 H2O (l)

A) 2.25
B) 1.13
C) 2.00
D) 4.50
E) none of the above

Answer: D

How many mL of 0.112 M Pb(NO3)2 are needed to completely react with 25.0mL of 0.105 M KI?

Given Pb(N )2(aq) + 2KI(aq) ? Pb (s) + 2KN (aq)

A) 11.7
B) 23.4
C) 0.147
D) 5.85
E) none of the above

Answer: A

What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L?

A) 1.67
B) 0.600
C) 0.0167
D) 3.0
E) none of the above

Answer: B

Which of the following aqueous solutions has the highest molar concentration of Na+ (aq)?

(Assume each compound is fully dissolved in water.)

A) 3.0M NaCl (sodium chloride)
B) 3.0M NaC2H3O2 (sodium acetate)
C) 1.5M Na2SO4 (sodium sulfate)
D) 1.0M Na3PO4 (sodium phosphate)
E) All of these solutions have the same concentration of Na+ (aq).

Answer: E

What volume (L) of 2.00 M KCl solution contains 25.0 g of KCl?

A) 0.335
B) 0.168
C) 0.672
D) 1.49
E) none of the above

Answer: B

How many grams of KCl are present in 75.0 mL of 2.10 M KCl?

A) 5.59
B) 117
C) 2.66
D) 11.7
E) none of the above

Answer: D

How many moles of KCl are present in 95.3 mL of KCl?

A) 0.0500
B) 5.00
C) 20.0
D) 0.200
E) none of the above

Answer: D

Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500. mL.

A) 0.331
B) 0.663
C) 0.166
D) 6.04
E) none of the above

Answer: B

Calculate the molarity of a KCl solution prepared by dissolving 0.525 moles of KCl in 250. mL of water.

A) 0.476
B) 0.00210
C) 2.10
D) 2.02
E) none of the above

Answer: C

Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water.

A) 27.3
B) 72.3
C) 47.0
D) 37.6
E) none of the above

Answer: A

What is the volume of 28.0 g of nitrogen gas at STP?

A) 33.6 L
B) 11.2 L
C) 22.4 L
D) 44.8 L
E) none of the above

Answer: C

What is the pressure of a 1.0 L flask containing 0.60 g of He at 25°C? (R= 0.0821 L atm/ mol K)

A) 98 atm
B) 3.7 atm
C) 7.3 atm
D) 15 atm
E) none of the above

Answer: B

What is the molecular weight of a gas if a 21.0 g sample has a pressure of 836 mm Hg at 25.0°C in a 2.00 L flask? (R= 0.0821 L atm/ mol K)

A) 243 amu
B) 1.89 amu
C) 234 amu
D) 11.1 amu
E) none of the above

Answer: C

What is the volume (in liters) of 1.00 mole of krypton gas that has a pressure of 1140 mm Hg and a temperature of 25.0°C? (R= 0.0821 L atm/ mol K)

A) 1.37
B) 16.3
C) 0.0215
D) 0.00180
E) none of the above

Answer: B

If the number of moles of a gas initially contained in a 2.10 L vessel is doubled, what is the final volume of the gas in liters? (Assume the pressure and temperature remain constant.)

A) 6.30
B) 1.05
C) 4.20
D) 8.40
E) none of the above

Answer: C

A rigid cylinder contains 2.00 liters of gas at a temperature of 25°C. If the pressure of this gas is changed from 0.500 atmospheres to 1.50 atmospheres, what will be the new temperature (in Kelvin, reported to three significant figures) of the gas? (The volume is constant.)

A) 99.3 K
B) 75.0 K
C) 8.33 K
D) 894 K
E) none of the above

Answer: D

What is the final pressure (expressed in atm) of a 3.05 L system initially at 724 mm Hg and 298 K, that is compressed to a final volume of 2.51 L at 273K?

A) 1.06
B) 1.60
C) 806
D) 860
E) none of the above

Answer: A

What is the final volume (L) of a 1.00 L system at 315 K and 1.10 atm if STP conditions are established?

A) 1.05
B) 0.935
C) 1.50
D) 0.953
E) none of the above

Answer: D

What is the change in temperature of a 2.50 L system when its volume is reduced to 1.75 L if the initial temperature was 298 K?

A) 209 K
B) 290 K
C) -89 K
D) -98 K
E) none of the above

Answer: C

What is the final volume of a gas that initially occupies 2.50 L at 298 K and is subsequently heated to 321 K?

A) 2.69 L
B) 2.96 L
C) 2.23 L
D) 2.32 L
E) none of the above

Answer: A

What is the final volume (L) of a 10.0 L system that has the pressure quartered?

A) 0.250
B) 17.1
C) 2.50
D) 40.0
E) none of the above

Answer: D

What is the final pressure of a system (atm) that has the volume increased from 0.75 L to 1.1 L with an initial pressure of 1.25 atm?

A) 1.1
B) 0.85
C) 1.8
D) 1.2
E) none of the above

Answer: B

What is the pressure of 760 mm Hg when expressed in units of in Hg?

A) 29.92 in Hg
B) 101,325 in Hg
C) 760 in Hg
D) 1 in Hg
E) none of the above

Answer: A

How many liters of O2 (g) are needed to react completely with 56.0 L of CH4 (g) at STP to produce CO2 (g) and H2O (g)?

Given CH4 (g) + 2O2 (g) ? CO2 (g) + H2O (g)

A) 28.0 L
B) 56.0 L
C) 84.0 L
D) 112. L
E) none of the above

Answer: D

Water can be formed according to the equation 2H2 (g) + O2 (g) ? 2H2O (g) If 8.0 L of hydrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction?

Water can be formed according to the equation
2H2 (g) + O2 (g) ? 2H2O (g)
If 8.0 L of hydrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction?

A) 4.0 L
B) 2.0 L
C) 1.0 L
D) 8.0 L
E) none of the above

Answer: A

If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?

Ammonia gas decomposes according to the equation
2NH3(g) ? N2(g) + 3H2(g)

If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?

A) 15.0 L
B) 30.0 L
C) 45.0 L
D) 90.0 L
E) not enough information

Answer: C

Suppose you had a balloon containing 1 mole of helium at STP and a balloon containing 1 mole of oxygen at STP. Which statement is TRUE?

A) The balloons will have the same volume.
B) The balloons will have the same mass.
C) Both A) and B) are true.
D) Neither A) nor B) are true.
E) not enough information

Answer: A

At STP, 12.69 g of a noble gas occupies 14.09 L. What is the identity of the noble gas? (R= 0.0821 L atm/ mol K)

At STP, 12.69 g of a noble gas occupies 14.09 L. What is the identity of the noble gas?
(R= 0.0821 L atm/ mol K)

A) He
B) Ne
C) Ar
D) Kr
E) not enough information

Answer: B

Which set of conditions reflect STP?

A) 298 K, 1 atm
B) 25°C, 14.7 psi
C) 373 K, 760 torr
D) 273 K, 1 Pa
E) 273 K, 760 mm Hg

Answer: E

Suppose a chemical reaction generated a 50% nitrogen/50% oxygen (by volume) mixture of gas that had a total volume of 22.4 liters at STP. This gas sample is composed of

A) 1 mole of nitrogen and 1 mole of oxygen.
B) 0.5 mole of nitrogen and 0.5 mole of oxygen.
C) 50 mole of nitrogen and 50 mole of oxygen.
D) 28 mole of nitrogen and 32 mole of oxygen.
E) none of the above

Answer: B

Hydrogen gas produced in the laboratory by the reaction of zinc and hydrochloric acid was collected over water at 25°C. The barometric pressure at the time was 742.5 mm Hg. What is the pressure of dry hydrogen gas if the vapor pressure of water at 25°C is 23.8 mm Hg?

A) 742.5 mm Hg
B) 718.7 mm Hg
C) 766.3 mm Hg
D) 760.0 mm Hg
E) none of the above

Answer: B

The vapor pressure of water at 20.0°C is 17.5 mm Hg. If the pressure of a gas collected over water was measured to be 453.0 mm Hg. What is the pressure of the pure gas?

A) 0.0230 atm
B) 0.619 atm
C) 0.573 atm
D) 0.596 atm
E) none of the above

Answer: C

Human lungs have evolved to breathe oxygen at a pressure as that in the atmosphere, 0.21 atm. If a particular heliox mixture to be carried by a scuba diver is at a pressure of 7.00 atm, what should be the partial pressure due to helium in order to maintain the pressure due to oxygen at 0.21 atm?

A) 0.21 atm
B) 7.00 atm
C) 6.79 atm
D) 7.21 atm
E) none of the above

Answer: C

What problem could happen if deep sea divers used pure oxygen in their tanks?

A) hypoxia
B) oxygen toxicity
C) nitrogen narcosis
D) rapture of oxygen
E) none of the above

Answer: B

A "shielding gas" mixture of argon and carbon dioxide is sometimes used in welding to improve the strength of the weld. If a gas cylinder of this two-part mixture was at 4.0 atm pressure and this mixture was 90.% argon, what would be the pressure due to the carbon dioxide gas component?

A) 3.6 atm
B) 0.40 atm
C) 10. atm
D) 4.0 atm
E) none of the above

Answer: B

A gas cylinder contains only the gases radon, nitrogen, and helium. The radon has a pressure of 222 torr while the nitrogen has a pressure of 446 torr. If the total pressure inside the cylinder is 771 torr, what is the pressure that is due to the helium?

A) 771 torr
B) 668 torr
C) 549 torr
D) 103 torr
E) none of the above

Answer: D

If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxide at 345 torr, what is the total pressure of the system?

A) 1,329 atm
B) 17.5 cm Hg
C) 639 torr
D) 1.75 atm
E) none of the above

Answer: D

What is the third most abundant component of dry air?

A) carbon dioxide
B) oxygen
C) nitrogen
D) argon
E) smog

Answer: D

What is the major component of the air we breathe?

A) nitrogen
B) oxygen
C) argon
D) carbon dioxide
E) smog

Answer: A

Which of the following diatomic elements would have a mass of 19.08 grams stored in a 3.82 L container at 3,632 mm Hg and 100°C? (R= 0.0821 L atm/ mol K)

A) H2
B) Br2
C) F2
D) O2
E) not enough information.

Answer: D

A 3.76 g sample of a noble gas is stored in a 2.00 L vessel at 874 torr and 25°C. What is the noble gas? (R= 0.0821 L atm/ mol K)

A 3.76 g sample of a noble gas is stored in a 2.00 L vessel at 874 torr and 25°C. What is the noble gas?
(R= 0.0821 L atm/ mol K)

A) He
B) Ne
C) Ar
D) Kr
E) not enough information

Answer: C

Which conditions can cause nonideal gas behavior by 1) decreasing the space between gas particles or 2) by slowing gas particles so that interactions are significant?

A) 1) high pressure; 2) high temperature
B) 1) high pressure; 2) low temperature
C) 1) low pressure; 2) high temperature
D) 1) low pressure; 2) low temperature
E) none of the above

Answer: B

What is the temperature (°C) of 2.48 moles of gas stored in a 30.0 L container at 1559 mm Hg? (R= 0.0821 L atm/ mol K)

What is the temperature (°C) of 2.48 moles of gas stored in a 30.0 L container at 1559 mm Hg?
(R= 0.0821 L atm/ mol K)

A) 302
B) 189
C) 29
D) -84
E) none of the above

Answer: C

What is the pressure of a 3.00 L gas vessel that has 18.0 grams of helium at 25 C? (R= 0.0821 L atm/ mol K)

A) 147 atm
B) 36.7 atm
C) 32.6 atm
D) 1.81 atm
E) none of the above

Answer: B

A sample of 0.255 mole of gas has a volume of 748 mL at 28°C. Calculate the pressure of this gas. (R= 0.0821 L · atm / mol · K)

A) 8.42 atm
B) 0.784 atm
C) 0.00842 atm
D) 7.84 × 10-4 atm
E) none of the above

Answer: A

The ideal gas law is

A) PV = nRT
B) P = nRT/V
C) T = PV/nR
D) V = nRT/P
E) All of the above are forms of the ideal gas law.

Answer: E

For an ideal gas, which of the following pairs of variables are inversely proportional to each other (if all other factors remain constant)?

A) P, V
B) P, T
C) V, T
D) n, P
E) none of the above

Answer: A

Which of the following gas law relationships is true?

A) V a 1/P
B) V a T
C) V a n
D) all of the above are true
E) none of the above are true

Answer: D

If each of the following gas samples have the same temperature and pressure, which sample has the greatest volume?

A) 1 gram of O2
B) 1 gram of Ar
C) 1 gram of H2
D) all have the same volume
E) not enough information

Answer: C

How many moles of gas were added to a balloon that started with 2.3 moles of gas and a volume of 1.4 L given that the final volume was 7.2 L?

A) 9.5
B) 4.4
C) 12
D) 0.085
E) none of the above

Answer: A

What happens to the volume of a gas when you double the number of moles of gas while keeping the temperature and pressure constant?

A) The volume is halved.
B) The volume doubles.
C) The volume decreases, but more information is needed.
D) The volume increases, but more information is needed.
E) none of the above

Answer: B

To solve problems using Avogadro's Law, which mathematical equation should be used?

A) n1/P1 = n2/P2
B) n1V1 = n2V2
C) V1/n1 = V2/n2
D) P1V1 = P2V2
E) none of the above

Answer: C

Avogadro's Law is expressed as

A) V is proportional to 1/n
B) P is proportional to n
C) n is proportional to 1/T
D) V is proportional to n
E) none of the above

Answer: D

What is the initial temperature (°C) of a system that has the pressure decreased by 10 times while the volume increased by 5 times with a final temperature of 150 K?

A) 27
B) 75
C) -198
D) 300
E) none of the above

Answer: A

What is the final volume of a 500.0 mL gas container that increased in temperature from 299 K to 333 K while the pressure increased from 1.00 atm to 1.54 atm?

A) 0.691 L
B) 2.77 L
C) 0.362 L
D) 1.45 L
E) none of the above

Answer: C

A sample of helium gas initially at 37.0°C, 785 torr and 2.00 L was heated to 58.0°C while the volume expanded to 3.24L. What is the final pressure in atm?

A) 517
B) 0.681
C) 1.79
D) 3.21
E) none of the above

Answer: B

A 325 mL sample of gas is initially at a pressure of 721 torr and a temperature of 32°C. If this gas is compressed to a volume of 286 mL and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in °C)?

A) 35.2°C
B) 335°C
C) 62.4°C
D) 215°C
E) none of the above

Answer: C

If the initial pressure of a system was 1.00 atm and the volume was halved and the kelvin temperature was tripled, what is the final pressure?

A) 2.00 atm
B) 0.667 atm
C) 1.50 atm
D) 6.00 atm
E) not enough information

Answer: D

Suppose a balloon was released from the ground and rose to such a height that both the atmospheric pressure and atmospheric temperature decreased. Which statement is TRUE?

A) Both the temperature and pressure changes act to increase the balloon's volume.
B) Both the temperature and pressure changes act to decrease the balloon's volume.
C) The temperature change acts to increase the balloon's volume.
D) The pressure change acts to decrease the balloon's volume.
E) none of the above

Answer: E

A certain volume of gas was confined in a rigid container. If the pressure of the gas sample in the container was doubled, what happened to the temperature?

A) The Kelvin temperature decreased by one-half.
B) The Kelvin temperature doubled.
C) The Kelvin temperature increased four times.
D) The Kelvin temperature decreased one-third.
E) not enough information

Answer: B

What is the proper form of the combined gas law?

A) P1T1/V1 = P2T2/V2
B) V1T1/P1 = V2T2/P2
C) P1V1/T1 = P2V2/T2
D) P1V1T1 = P2V2T2
E) none of the above

Answer: C

Which of the following statements is TRUE for gases? 1. The temperature of a gas is inversely proportional to its pressure. 2. The volume of a gas is directly proportional to the pressure in torr. 3. The pressure of a gas is due to collisions of the gas molecules.

Which of the following statements is TRUE for gases?
1. The temperature of a gas is inversely proportional to its pressure.
2. The volume of a gas is directly proportional to the pressure in torr.
3. The pressure of a gas is due to collisions of the gas molecules.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2 only
E) 1 and 3 only

Answer: C

Gas density can be calculated by dividing the mass of gas by its volume. If you took a balloon of gas and then warmed the balloon in a sunny window, what can now be said about the density of the gas in the balloon?

A) The gas density will remain the same.
B) The gas density will increase.
C) The gas density will decrease.
D) The density of gases is independent of temperature.
E) none of the above

Answer: C

A balloon originally had a volume of 0.439 L at 44°C and a pressure of 729 torr. To what temperature must the balloon be cooled to reduce its volume to 378 mL if the pressure remained constant?

A) 0°C
B) 38°C
C) 95°C
D) 273°C
E) none of the above

Answer: A