Chemistry Final

What type of inhibitor binds to the enzyme but does not bind at the active site? a. A noncompetitive inhibitor b. A competitive inhibitor c. A reversible inhibitor d. An irreversible inhibitor

a. A noncompetitive inhibitor

What is the process of altering the shape of a protein without breaking the amide bonds that form the primary structure? a. Hydrolysis b. Competitive inhibition c. Denaturation d. Oxidation

c. Denaturation

When forming ions, metals typically do which of the following? Select one: a. Gain protons to form cations b. Lose electrons to form negatively charged ions c. Lose electrons to form positively charged ions d. Gain electrons to form anions

c. Lose electrons to form positively charged ions

How many significant figures does the result of the following sum contain? 8.520 + 2.7 a. 2 b. 4 c. 5 d. 1 e. 3

e. 3

The number 1.050 × 109 has how many significant figures? Select one: a. 13 b. 9 c. 3 d. 2 e. 4

e. 4

How many valence electrons does P3- have? a. 18 b. 15 c. 3 d. 1 e. 8

e. 8

Name the compound CuSO4 a. Copper (I) sulfite b. Copper (II) sulfate c. Copper (II) sulfite d. Copper (IV) sulfate e. Copper (I) sulfate

b. Copper (II) sulfate

Which species is the conjugate acid of HCO3-? a. CO32- b. H2CO3 c. CO2 d. H2O

b. H2CO3

What is the best antacid (per dose)? Select one: a. Tums b. Rolaids c. Alka-Seltzer d. Hydrochloric acid

b. Rolaids

What are the two different ions present in the compound Li3N? Select one: a. Li+, N- b. Li3+, N3- c. Li3+, N- d. Li+, N3- e. Li33+, N3-

d. Li+, N3-

A piece of metal with a mass of 611 g is placed into a graduated cylinder that contains 25.1 mL of water, raising the water level to 56.7 mL. What is the density of the metal? (1mL = 1cm3) a. 7.13 g/cm3 b. 2.70 g/cm3 c. 8.96 g/cm3 d. 10.5 g/cm3 e. 19.3 g/cm3

e. 19.3 g/cm3

What is the formula for the ionic compound containing calcium ions and nitrate ions? a. Ca2NO2 b. CaNO3 c. Ca2NO3 d. Ca3N2 e. Ca(NO3)2

e. Ca(NO3)2

An atom of the isotope 137Ba consists of how many protons (p), neutrons (n), and electrons (e)? a. 56 p, 81 n, 56 e b. 56 p, 137 n, 56 e c. 81 p, 56 n, 81 e d. 56 p, 56 n, 56 e e. 137 p, 81 n, 56 e

a. 56 p, 81 n, 56 e

Which one of the following is most likely to be a covalent compound? a. SF4 b. Al2O3 c. KF d. CaCl2 e. CaSO4

a. SF4

The small molecule N2 can move in and out of cells primarily by which of the following? a. passive transport b. facilitated transport c. active transport d. tertiary transport

a. passive transport

How many milliliters is 0.005 L? a. 200 mL b. 0.50 mL c. 5 mL d. 0.000005 mL e. 0.5 mL

c. 5 mL

Which one of the following represents a physical change? a. sugar, when heated, becomes brown b. bleach turns hair yellow c. water, when heated to 100°C, forms steam d. milk turns sour e. apples, when exposed to air, turn brown

c. water, when heated to 100°C, forms steam

Beta particles are identical to a. helium atoms. b. protons. c. hydrogen atoms. d. electrons. e. helium nuclei.

d. electrons.

Atoms of the same element with different mass numbers are called a. ions. b. neutrons. c. chemical families. d. isotopes e. allotropes.

d. isotopes

The elements in a column of the periodic table are known as a. nonmetals. b. metalloids. c. a period. d. noble gases. e. a group.

e. a group.

Which one of the following elements forms a stable 2+ cation? a. Ba b. I c. Se d. Al e. Kr

a. Ba

Hemoglobin the protein cannot bind O2 by itself, rather it requires _____________ which binds O2. a. NADH b. Heme c. CO2 d. Mg2+ e. glucose

b. Heme

A sample of neon gas has a volume of 5.0 mL at a pressure of 1.50 atm. What is the pressure exerted by the gas if the volume is increased to 30.0 mL, at constant temperature? a. 0.25 atm b. 9.0 atm c. 1.5 atm d. 0.21 atm

a. 0.25 atm

The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present in one 500-milligram tablet? a. 1.67 × 1021 molecules b. None of these is correct. c. 2.77 × 10-3 molecules d. 1.67 × 1024 molecules e. 2.77 molecules

a. 1.67 × 1021 molecules

The density of lead is 11.4 g/cm3 at 25°C. Calculate the volume occupied by 25.0 g of lead. a. 2.19 cm3 b. 1.24 cm3 c. 285 cm3 d. 6.05 cm3 e. 0.456 cm3

a. 2.19 cm3

How many milliliters of a 5.25% (w/v) HCl solution must be used to prepare 250 mL of a 0.175% (w/v) HCl solution? a. 8.3 mL HCl solution b. 240 mL HCl solution c. 7,500 mL HCl solution d. 8.6 mL HCl solution e. 230 mL HCl solution

a. 8.3 mL HCl solution

A particular wine contains 11.2% (v/v) ethanol. What volume of ethanol is in a 750.-mL bottle of this wine? a. 84.0 mL ethanol b. 0.840 mL ethanol c. 6.70 mL ethanol d. 14.9 mL ethanol

a. 84.0 mL ethanol

Which statement is not true? a. A coenzyme is a metal ion needed for an enzyme-catalyzed reaction to occur. b. Enzymes must bind one or more substrates in order to catalyze a reaction. c. An enzyme-catalyzed reaction is faster than a similar uncatalyzed reaction. d. Enzymes are proteins that serve as biological catalysts for reactions in all living organisms.

a. A coenzyme is a metal ion needed for an enzyme-catalyzed reaction to occur.

Which pair of compounds will form a solution? Select one: a. Benzene (C6H6) and hexane (C6H14) b. Na2SO4 and benzene (C6H6) c. NaCl and hexane (C6H14) d. H2O and CCl4 e. More than one of the combinations above will form solutions.

a. Benzene (C6H6) and hexane (C6H14)

Which gas law describes the relationship between the volume and temperature of a sample of gas at constant pressure? a. Boyle's law b. Avogadro's law c. Charles's law d. Gay-Lussac's law

a. Boyle's law

Which is the first stage of catabolism in humans? a. Digestion b. Citric acid cycle c. Fatty acid oxidation d. Glycolysis e. Formation of acetyl CoA

a. Digestion

Which of the following is *not* a strong acid? a. HClO2 b. HCl c. sulfuric acid d. nitric acid e. HBr

a. HClO2

At rest, the volume of air in the lungs is 615 mL at 760 mm Hg. When the volume of the lungs expands during inhalation, what happens to the pressure inside the lungs? a. The pressure inside the lungs decreases, which draws air into the lungs. b. The pressure inside the lungs increases, which forces air inside the lungs. c. The pressure inside the lungs remains constant, and air readily flows into the lungs. d. The pressure inside the lungs cannot be determined if the weight of the person is unknown.

a. The pressure inside the lungs decreases, which draws air into the lungs.

What is the particular sequence of amino acids of a protein that are joined together by peptide bonds called? a. The primary structure of a protein b. The secondary structure of a protein c. The tertiary structure of a protein d. The quaternary structure of a protein

a. The primary structure of a protein

When is pyruvate converted to acetyl CoA? a. Under aerobic conditions b. Under anaerobic conditions c. During fermentation d. This conversion is favorable under all of the conditions above.

a. Under aerobic conditions

Which one of the following elements is a transition metal? Select one: a. chromium (Cr) b. barium (Ba) c. selenium (Se) d. antimony (Sb) e. potassium (K)

a. chromium (Cr)

LDL, HDL, and chylomicrons are used to transport ________________ in the _______________. a. lipids, blood b. proteins, blood c. carbohydrate, blood d. lipid, mitochondria e. protein, mitochondria f. carbohydrate, mitochondria

a. lipids, blood

What is the concentration of a solution formed by diluting 25.0 mL of a 3.2 M NaCl solution to 135.0 mL? a. 17 M NaCl b. 0.59 M NaCl c. 0.50 M NaCl d. 2.7 M NaCl

b. 0.59 M NaCl

How many reactions in the citric acid cycle generate FADH2? a. 0 b. 1 c. 2 d. 3 e. 4

b. 1

The maximum level of lead allowed in drinking water is 15 μg/kg. What is this concentration in units of parts per million? a. 15 ppm b. 1.5 × 10-2 ppm c. 1.5 × 104 ppm d. 3.1 ppm

b. 1.5 × 10-2 ppm

Which of the following are isotopes? a. 14N and 14N3- b. 14C and 13C c. 14N and 14N2 d. 12C and 12CO e. 14C and 14N

b. 14C and 13C

The total number of valence electrons in the molecule CO2 is Select one: a. 4 b. 16 c. 14 d. 20 e. 10

b. 16

How many different dipeptides can be formed when one valine reacts with one glycine? a. 1 b. 2 c. 3 d. 4

b. 2

The breakdown of glucose in metabolism makes, a. 2 ATP, 2 FADH2 b. 2 ATP, 2 NADH c. 4 ATP, 4 NADH d. 4 ATP, 2 NADH

b. 2 ATP, 2 NADH

What is the net production of ATP from the complete breakdown of lauric acid (12-carbons) from coconut oil (don't forget to include activation step). a. 68 b. 78 c. 80 d. 86 e. 70

b. 78

How many equivalents are in a solution containing 3.09 moles of aluminum ions in 1.50 L of solution? a. 3.09 equivalents b. 9.27 equivalents c. 6.18 equivalents d. 0.673 equivalents

b. 9.27 equivalents

A Brønsted-Lowry acid is a. A compound that contains hydroxide and dissolves in water to form OH-. b. A compound that is a proton donor. c. A compound that is a proton acceptor. d. A compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

b. A compound that is a proton donor.

A hypotonic solution has _____ osmotic pressure than/as body fluids. a. A higher b. A lower c. The same

b. A lower

Which of the following statements concerning a solution is NOT true? a. A solution is a heterogeneous mixture of two or more pure substances. b. A solution is composed of a solvent and one or more solutes; the solute(s) dissolve in the solvent. c. A solution has its components uniformly distributed. d. A solution is likely to form when the solute(s) and the solvent have similar polarities.

b. A solution is composed of a solvent and one or more solutes; the solute(s) dissolve in the solvent.

Glycolysis converts _____ a. Polysaccharides to glucose. b. Glucose to pyruvate, which is then metabolized to acetyl CoA. c. Fatty acids to thioesters, which are metabolized to acetyl CoA. d. Amino acids to urea.

b. Glucose to pyruvate, which is then metabolized to acetyl CoA.

ATP is synthesized by Complex V also known as ATP synthase, which best describes the process? a. GTP from citric acid cycle powers ATP synthase. b. H+ from electron transport drive phosphorylation of ADP as they renter mitochondria c. electrons from electron transport directly powers ATP synthase d. acetyl-CoA binds the active site of Complex V catalyzing ATP synthesis

b. H+ from electron transport drive phosphorylation of ADP as they renter mitochondria

Which species can act as a Brønsted-Lowry acid? Select one: a. CO32- b. HBr c. Br2 d. LiOH

b. HBr

What interactions are responsible for holding dissolved Cl- ions in an aqueous solution? a. Ion-ion attractions between K+ and Cl- ions b. Ion-dipole attractions between Cl- ions and the hydrogen atoms of water c. Ion-dipole attractions between Cl- ions and the oxygen atom of water d. Hydrogen bonding between the Cl- ions and water

b. Ion-dipole attractions between Cl- ions and the hydrogen atoms of water

What is the strongest type of interaction between the side chains of an alanine (-CH3) and a serine (-CH2OH) in a protein? a. Hydrogen bonding b. London dispersion forces c. Disulfide bond d. Electrostatic interactions

b. London dispersion forces

How is a dipeptide formed? a. The -NH3+ group of one amino acid forms an amide bond with the -NH3+ group of another amino acid and the elements of H2 are removed. b. The -NH3+ group of one amino acid forms an amide bond with the carboxylate (-COO-) of another amino acid, and the elements of H2O are removed. c. The carboxylate (-COO-) group of one amino acid forms an amide bond with the carboxylate (-COO-) of another amino acid, and the elements of O2 are removed. d. The carboxylate (-COO-) group of one amino acid forms an amide bond the -NH3+ group of another amino acid, and the elements of H2 are removed.

b. The -NH3+ group of one amino acid forms an amide bond with the carboxylate (-COO-) of another amino acid, and the elements of H2O are removed.

The pH of normal blood is 7.4. The pH of a diabetic's blood was determined to be 6.4. Which comparison of these two blood samples is accurate? a. The diabetic's blood has a lower [H3O+] than normal blood. b. The diabetic's blood is more acidic than normal blood. c. Normal blood has a lower [OH-] than the diabetic's blood. d. Normal blood has a higher [H3O+] than the diabetic's blood.

b. The diabetic's blood is more acidic than normal blood.

Which of the statements concerning chemical bonds is false? a. The sharing of electrons between two nonmetal atoms results in a covalent bond. b. The term nonpolar is used to describe a covalent bond in which electrons are not shared equally. c. A bond dipole is the separation of charge that results when atoms sharing electrons have different electronegativities. d. The attraction between oppositely charged ions results in an ionic bond.

b. The term nonpolar is used to describe a covalent bond in which electrons are not shared equally.

Which statement describing atoms is false? a. Electrons are located in the space outside the nucleus called the electron cloud. b. The total number of protons, neutrons, and electrons in an atom is referred to as the mass number of the atom. c. Protons and neutrons are located in the nucleus of an atom. d. The number of protons in an atom is referred to as the atomic number of the atom.

b. The total number of protons, neutrons, and electrons in an atom is referred to as the mass number of the atom.

A sample of water from the Missouri river has [H3O+]=3.1 × 10-9 M. Which statement below accurately describes this water sample? a. The pH of the water sample is 7.5. b. The water sample is a basic solution. c. The water sample doesn't contain any hydroxide ions. d. The water sample has a higher concentration of hydronium ions than pure water does.

b. The water sample is a basic solution.

If cells are placed in a hypertonic solution, a. Water diffuses out of the cells and the cells shrink in a process called hemolysis. b. Water diffuses out of the cells and the cells shrink in a process called crenation. c. Water diffuses into the cells and the cells swell and eventually burst in a process called hemolysis. d. Water diffuses into the cells and the cells swell and eventually burst in a process called crenation.

b. Water diffuses out of the cells and the cells shrink in a process called crenation.

Name the compound N2O4 a. nitrous oxide b. dinitrogen tetroxide c. dinitrogen pentoxide d. nitrogen oxide e. nitrogen tetroxide

b. dinitrogen tetroxide

Classify the O — H bond in CH3OH as ionic, polar covalent, or nonpolar covalent. (Electronegativies: C-2.5, O-3.5, H-2.1) a. nonpolar covalent b. polar covalent c. ionic

b. polar covalent

Normal gastric juice has a pH of about 2. Assuming that normal gastric juice is primarily aqueous HCl, what is the concentration of HCl in the stomach? a. 2 M HCl b. 1.0 × 102 M HCl c. 0.01 M HCl d. 0.14 M HCl

c. 0.01 M HCl

A patient's systolic pressure is measured as 128 mm Hg. What is this pressure in units of atm? a. 128 atm b. 1.28 atm c. 0.168 atm d. 9.73 x 104 atm

c. 0.168 atm

What is the molarity of a solution made by dissolving 36.29 g of NaCl in 2.30 L of solution? a. 15.78 M NaCl b. 0.0634 M NaCl c. 0.270 M NaCl d. 2.70 M NaCl

c. 0.270 M NaCl

Which solution has the highest pH? a. 4.3 × 10-8 M -OH b. 1.9 × 10-8 M -OH c. 1.0 × 10-7 M -OH d. 1.0 × 10-2 M H3O+ e. 5.1 × 10-2 M H3O+

c. 1.0 × 10-7 M -OH

What fraction of radioactive atoms remains in a sample after six half-lives? Select one: a. zero b. 1/16 c. 1/64 d. 1/32 e. 1/6

c. 1/64

What is the molar mass of acetaminophen, C8H9NO2? a. 135.16 g/mol b. 143.10 g/mol c. 151.16 g/mol d. 67.09 g/mol e. 43.03 g/mol

c. 151.16 g/mol

How many molecules of CO2 are produced for each turn of the citric acid cycle? a. 0 b. 1 c. 2 d. 3 e. 4

c. 2

How many C atoms are in 5.50 g of C? a. 5.01 x 1022 C atoms b. 6.02 x 1023 C atoms c. 2.76 x 1023 C atoms d. 3.31 x 1024 C atoms e. 5.50 x 1023 C atoms

c. 2.76 x 1023 C atoms

A solution is made by mixing 569 mL of water and 238 mL ethanol. What is the concentration of ethanol in units of volume/volume percent? a. 41.8% (v/v) ethanol b. 0.418% (v/v) ethanol c. 29.5% (v/v) ethanol d. 0.295% (v/v) ethanol e. 70.5% (v/v) ethanol

c. 29.5% (v/v) ethanol

A saline solution used in intravenous drips for patients who cannot take oral fluids contains 0.92% (w/v) NaCl in water. How many grams of NaCl are contained in 575 mL of this solution? a. 53 g NaCl b. 529 g NaCl c. 5.3 g NaCl d. 0.016 g NaCl e. 1.6 g NaCl

c. 5.3 g NaCl

If the half-life of phosphorus-32 is 14.3 days, how much of a 200. mg sample of phosphorus-32 remains after 71.5 days? a. 100. mg b. 50. mg c. 6.25 mg d. 12.5 mg

c. 6.25 mg

How many reactions make up the citric acid cycle? a. 3 b. 6 c. 8 d. 9 e. 10

c. 8

Which is an example of a globular (spherical) protein? a. Collagen b. Triacylglycerol c. Hemoglobin d. Amylopectin

c. Hemoglobin

Which of the following choices lists all the intermolecular forces possible for pure methanol? a. London dispersion only b. London dispersion, dipole-dipole c. London dispersion, dipole-dipole, hydrogen bonding d. London dispersion, dipole-dipole, hydrogen bonding, ion-dipole e. hydrogen bonding only

c. London dispersion, dipole-dipole, hydrogen bonding

Denaturation of a protein results in the loss of its native conformation and its biological activity. Which statement best describes what happens to a protein when it is denatured? a. Peptide bonds are broken. b. New amino acids are joined to the peptide backbone. c. Secondary, tertiary, and quaternary levels of structure are disrupted. d. The N-terminal and C-terminal ends of the protein are hydrolyzed by enzymes.

c. Secondary, tertiary, and quaternary levels of structure are disrupted.

Tuftsin is a peptide that stimulate and promotes the destruction of tumor cells. Its primary structure is Thr-Lys-Pro-Arg. Which statement is NOT a valid interpretation of its primary structure? a. It is a tetrapeptide. b. Threonine is the N-terminal amino acid and arginine is the C-terminal amino acid. c. The amino group of arginine is not joined to any other amino acid. d. The carboxyl group of lysine is joined to the amino group of proline.

c. The amino group of arginine is not joined to any other amino acid.

An aerosol spray can with a volume of 350 mL registers a pressure of 4.5 atm at room temperature. What happens to the pressure of the gas inside the can if the can is stored outside during the winter months? a. The pressure of the gas will remain at 4.5 atm. b. The pressure of the gas will be greater than 4.5 atm. c. The pressure of the gas will be less than 4.5 atm. d. It is impossible to predict without knowing the amount of gas present inside the can.

c. The pressure of the gas will be less than 4.5 atm.

Predict the molecular geometry and polarity of the SO2 molecule. (Electronegativities: S-2.5, O-3.5) a. bent, nonpolar b. linear, nonpolar c. bent, polar d. linear, polar e. None of the answers listed is correct

c. bent, polar

The level of protein structure that corresponds to the overall shape or fold of a single polypeptide chain is, a. primary b. secondary c. tertiary d. quaternary e. pentanary

c. tertiary

The primary function of the electron transport chain and oxidative phosphorylation is which of the following? a. to provide electrons and energy for the phosphorylation of ATP b. to synthesize the reduced coenzymes necessary for digestion c. to oxidize the reduced coenzymes NADH and FADH2, and provide energy for the synthesis of ATP d. to transport electrons from ATP to ADP, and synthesize acetyl CoA molecules

c. to oxidize the reduced coenzymes NADH and FADH2, and provide energy for the synthesis of ATP

An aluminum beverage can contain 12.0 fluid ounces of liquid. Express this volume in liters. (1 fl oz = 29.6 mL) a. 3.55 × 102 L b. 2.46 L c. 0.407 L d. 0.355 L e. 4.07 × 10-2 L

d. 0.355 L

An aqueous solution with a low pH is necessary for a certain industrial process. Which of the following solutions would have the lowest pH? a. 2.0 M NaOH b. 0.5 M HCl c. 0.15 M NaOH d. 1.0 M HCl e. 1.0 M acetic acid, CH3COOH

d. 1.0 M HCl

The number of lone (non-bonding) electron pairs in the N2 molecule is ___. a. 5 b. 4 c. 1 d. 2 e. 3

d. 2

Express the number 26.7 in scientific notation. a. 2.67 × 102 b. 2.67 × 10-1 c. 2.67 × 10-2 d. 2.67 × 101 e. 26.7 is already written in scientific notation

d. 2.67 × 101

An oxide ion, O2-, has: a. 10 protons and 7 electrons b. 10 protons and 8 electrons c. 8 protons and 7 electrons d. 8 protons and 10 electrons e. 8 protons and 9 electrons

d. 8 protons and 10 electrons

_____ are negatively charged ions that have _____ electrons than protons. a. Anions, less b. Cations, more c. Cations, less d. Anions, more

d. Anions, more

Fats and oils are similar, but fats are solids at room temperature and oils are liquids at room temperature. Which statement best describes the reason for their difference in physical state? a. Fats are triacylglycerols and oils are fatty acids. b. Oils are triacylglycerols and fats are fatty acids. c. Oils contain longer fatty acid chains than fats do, and therefore have higher melting points than fats. d. Fats contain a higher percentage of saturated fatty acids than oils do, and therefore have higher melting points than oils.

d. Fats contain a higher percentage of saturated fatty acids than oils do, and therefore have higher melting points than oils.

Which one of the following is most likely to be an ionic compound? a. NH3 b. PF3 c. ClF3 d. FeCl3 e. SO3

d. FeCl3

Which molecule(s) exhibit hydrogen bonding? a. CH4 b. CHCl3 c. NF3 d. HF e. All of the molecules above exhibit hydrogen bonding.

d. HF

About one half of the 223 amino acid residues in the enzyme trypsin are hydrophobic. Where in the tertiary structure of this globular protein are these residues most likely to be found? a. At the N-terminal end of the peptide chain. b. At the C-terminal end of the peptide chain. c. On the exterior surface of the folded protein. d. In the interior of the folded protein.

d. In the interior of the folded protein.

Nonpolar compounds are soluble in a. Ionic compounds. b. Electrolytes. c. Polar solvents. d. Nonpolar solvents.

d. Nonpolar solvents.

Ammonia, NH3, is an example of a a. Strong acid b. Strong base c. Weak acid d. Weak base

d. Weak base

An anion is defined as a. a group of stable atoms. b. a stable atom. c. an atom or group of atoms with a net positive charge. d. a charged atom or group of atoms with a net negative charge.

d. a charged atom or group of atoms with a net negative charge.

List the different types of nuclear radiation (alpha, beta, gamma) in order of increasing penetrating power. a. alpha < gamma < beta b. gamma < beta < alpha c. gamma < alpha < beta d. alpha < beta < gamma e. beta < alpha < gamma

d. alpha < beta < gamma

Define electronegativity: a. an atoms ability to form an ionic bond with another atom b. an atoms ability to donate valence electrons to another atom c. an atoms ability to form double and triple bonds d. an atoms ability to attract electrons that are shared in a chemical bond e. an atoms ability to form a cation

d. an atoms ability to attract electrons that are shared in a chemical bond

In the electron transport chain, FADH2 enters at ____________ and NADH enters at _____________. a. complex, II, complex III b. complex I, complex II c. complex I, complex III d. complex II, complex I e. complex III, complex I

d. complex II, complex I

Give the number of lone pairs around the central atom and the molecular geometry of SCl2. a. 1 lone pair, bent b. 0 lone pairs, linear c. 3 lone pairs, bent d. 3 lone pairs, linear e. 2 lone pairs, bent

e. 2 lone pairs, bent

Which cylinder at 1 atm of pressure and 300 K will contain the greatest number of gas particles? a. A 5.0-L cylinder of neon b. A 5.0-L cylinder of helium c. A 5.0-L cylinder of nitrogen d. A 5.0-L cylinder of hydrogen e. All of the cylinders above contain the same number of gas particles.

e. All of the cylinders above contain the same number of gas particles.