5 CHEM1210 problems a day keeps the knowledge here to stay

Choose the name-formula pair that does not match: a) ammonium hydrogen carbonate, NH4CO3 b) sodium chlorite, NaClO2 c) calcium hydride, CaH2 d) nitric acid, HNO3 e) calcium hydroxide, Ca(OH)2

A

The formation of which monatomic ion of sulfur is the most energetically favorable? A) S4+ B) S2- C) S- D) S6+ E) 2+

B

The formula for copper (II) phosphate is: a) CuPO4 b) Cu3(PO4)2 c) Co3(PO4)2 d) Cu2(PO4)3 e) Co2(PO4)3

B

When a particular metal is illuminated with photons, one electron is observed for each absorbed photon. What effect would decreasing the wavelength and number of photons have on the electrons leaving the surface? a. There would be more electrons leaving the surface. b. They would have higher kinetic energy. c. The electron velocity would be lower. d. The kinetic energy of the electrons would be lower. e. Two photons might be required to eject the electrons.

B

Which of the following is/are MOLECULAR compounds? (i) CO (ii) NH4Br (iii) H2SO4 (iv) MnCl4 (v) XeCl4 a) (i), (ii), (iii) b) (i), (iii), (v) c) (i), (v) d) (i), (ii), (iii), (v) e) All

B

Which of the following matched pairs of name and formula has an error? a. LiClO2 lithium chlorite b. HIO3 periodic acid c. HClO2 chlorous acid d. HBrO hypobromous acid e. Sr(ClO4)2 strontium perchlorate

B

Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? A) H2O and HCl B) NO and NO2 C) NH4 and NH4Cl D) ZnO2 and ZnCl2 E) CH4 and CO2

B

Which one of the following samples has the greatest mass? 8.9 mol of krypton, Kr b) 4.5 mol of iodine vapor, I2 c) 3.5 mol of formaldehyde, CH2O d) 0.51 mol of camphor, C10H16O e) 3.4 mol of ammonia, NH3

B

A molecular compound contains 92.3 % carbon and 7.7 % hydrogen by mass. If 0.432 mol of the compound weighs 22.46 g, what is its molecular formula? A) C8H8 B) C6H10 C) C4H8 D) C4H4 E) CH

D

A particular compound contains, by mass, 41.4% carbon, 3.47% hydrogen, and 55.1% oxygen. A 0.050-mol sample of this compound weighs 5.80 g. The molecular formula of this compound is: a) CHO b) C3H3O c) C2H2O2 d) C4H4O4 e) C5H5O5

D

A sealed 22.4 L flask contains pure O2 at STP. A second sealed 22.4 L flask contains CH 4 at STP. Which of the following statements concerning the molecules in the flasks is/are true? 1. The average kinetic energy of the O 2 molecules is greater than the average kinetic energy of CH4 molecules. 2. The average velocity of the CH 4 molecules is greater than the average velocity of the O2 molecules. 3. The volume occupied by the gas molecules in both flasks is small relative to the total volume of the flasks. a. 1 only b. 2 only c. 3 only d. 2 and 3 e. 1, 2, and 3

D

A thin sheet of platinum metal that is 3.85 cm by 6.16 cm has a mass of 68.0 g and a thickness of 1.36 mm. What is the density of platinum? A) 2.19 *10^3 g/cm^3 B) 2.11 g/cm^3 C) 0.474 g/cm^3 D) 21.1 g/cm^3 E) 0.0474 g/cm^3

D

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) a. 97.4 mL b. 116 mL c. 43.0 mL d. 86.1 mL e. 58.1 mL

D

All the following may change during a chemical reaction except A) the total volume of the system. B) the density of the system. C) the temperature of the system. D) the total number of atoms in the system. E) the total number of molecules in the system.

D

An atom of which of the following elements is not diamagnetic in the ground state? a. Ba b. Kr c. Hg d. Pt e. All are diamagnetic.

D

Arrange the bonds in each of the following sets in order of decreasing polarity: C-F, O-F, Be-F a. C-F > O-F > Be-F b. O-F > Be-F > C-F c. O-F > C-F > Be-F d. Be-F > C-F > O-F e. Be-F > O-F > C-F

D

Determine the name for CoCl2·6H2O. a) cobalt chloride hydrate b) cobalt (I) chloride heptahydrate c) cobalt (II) chloride heptahydrate d) cobalt (II) chloride hexahydrate e) cobalt (I) chloride

D

Determine the name for CuSO4·5H2O. a) copper sulfate hydrate b) copper (I) sulfate pentahydrate c) copper (II) sulfate hexahydrate d) copper (II) sulfate pentahydrate e) copper (I) sulfate

D

For the reaction that occurs in a lead storage battery, Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4-(aq) → 2PbSO4(s) + 2H2O(l) the oxidizing agent is: a. HSO4- b. PbSO4 c. Pb d. PbO2 e. H+

D

From the following information, determine ∆H°f of malonic acid, CH2(COOH)2(s). CH2(COOH)2(s) + 2O2(g) → 3CO2(g) + 2H2O(l); ∆H° = -861.0 kJ Substance ∆H°f (kJ/mol) CO2(g) -393.5 H 2O(l) -285.8 a. -1540.3 kJ b. -2613.1 kJ c. 891.1 kJ d. -891.1 kJ e. 2613.1 kJ

D

A 100 g sample of each of the following metals is heated from 35°C to 45°C. Which metal absorbs the lowest amount of heat energy? Metal Specific Heat copper 0.385 J/(g · °C) magnesium 1.02 J/(g · °C) mercury 0.138 J/(g · °C) silver 0.237 J/(g · °C) lead 0.129 J/(g · °C) a. lead b. magnesium c. silver d. mercury e. copper

A

A 14.01 g sample of N 2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? a. 17.01 g b. 1.10 g c. 14.01 g d. 3.02 g e. 23.07 g

A

A car averages 27.5 miles per gallon of gasoline. How many liters of gasoline will be needed for a trip of 489 km? Some conversion factors that may be helpful are the following: 1 qt = 0.946 L 1 mile = 1.609 km 4 qt = 1 gal (exact) 1 ft = 12 in (exact) A) 4.18 × 10^1 L B) 5.72 × 10^3 L C) 2.21 × 10^3 L D) 1.08 × 10^2 L E) 3.16 × 10^4 L

A

A flexible container is charged with 51.00 L of gas at 368 Κ. Under conditions of constant pressure and moles of gas, what is the volume of the gas when the temperature is tripled? a. 153 L b. 17.0 L c. 0.0588 L d. 51 L e. 0.850 L

A

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution? a. 0.274 M b. 0.356 M c. 2.81 M d. 3.65 M e. 5.00 M

A

All of the following equations are balanced except: A) (NH4)2Cr2O7 → N2O + Cr2O3 + 4H2O B) 2NH4SCN + Ba(OH)2 • 8H2O → 2NH3 + 10H2O + Ba(SCN)2 C) C12H22O11 → 12C + 11H2O D) NH4NO3 → N2O + 2H2O E) 2Mg + CO2 → 2MgO + C

A

At constant pressure, the sign of q for the process CO2(s) → CO2(g) is expected to be: a. Positive, and the process is endothermic b. Negative, and the process is endothermic c. Positive, and the process is exothermic d. Negative, and the process is exothermic. e. Impossible to predict.

A

Calculate the enthalpy for the reaction: P4O6 (s) + 2O2 (g) à P4O10 (s) given the following enthalpies of reaction: P4 (s) + 3O2 (g) → P4O6 (s) ΔH1 = -1640.1 kJ P4 (s) + 5O2 (g) → P4O10 (s) ΔH2 = -2940.1 kJ a. -1300.0 kJ b. 1300 kJ c. -4580 kJ d. 4580 kJ e. 1300 J

A

Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP). 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g) a. 27.1 g, 80.4 % yield b. 179 g, 12.2 % yield c. 91.7 g, 23.8 % yield d. 206 g, 10.6 % yield e. 61.0 g, 35.7 % yield

A

Gallium has an atomic mass of 69.723 amu. The Ga-69 (68.926 amu) is 60.11%. What is the amu of the other isotope? a) 70.924 amu b) 70.928 amu c) 70.932 amu d) 70.920 amu e) 70.918 amu

A

How many grams of potassium ions are present in 21.6 g of K2Cr2O7? A) 5.74 g B) 1.105 g C) 2.87 g D) 78.2 g E) 10.8 g

A

How many protons, neutrons and electrons are in the Co3+ cation? a) 27, 32, 24 b) 59, 27, 27 c) 27, 32, 30 d) 27, 32, 27 e) 32, 27, 24

A

In 0.100 mol of dimethylhydrazine, (CH3)2N2H2, there are: a. 7.22 × 10^23 atoms b. 6.62 × 10^23 atoms c. 4.82 × 10^23 atoms d. 6.02 × 10^24 molecule e. 6.02 × 10^23 molecules

A

It is possible to make a barometer using a liquid other than mercury. What would be the height (in meters) of a column of water at a pressure of 0.390 atm, given that 0.390 atm is equal to a 0.296 m column of mercury and the densities of mercury and water are 13.5g/cm^3 and 1.00 g/cm^3, respectively. a. 4.00 m b. 0.250 m c. 0.0220 m d. 0.296 m e. 3.37 m

A

What is the total number of valence electrons in N2O4? a. 34 b. 11 c. 16 d. 17 e. 46

A

Which of the following combinations will produce a precipitate? 1. AgNO 3(aq) and HCl(aq) 2. HCl(aq) and Na2CO3(aq) 3. NaOH(aq) and K 3PO4(aq) a. 1 only b. 2 only c. 3 only d. 2 and 3 e. 1, 2, and 3

A

Which of the following is/are ionic compounds? (i) SCl2 (ii) Mg3(PO4)2 (iii) Cl2O (iv) LiCl (v) SeBr2 A. (ii) and (iv) B. (ii), (iv) and (v) C. (i), (ii), (iv) and (v) D. (i) and (ii) E. All of them

A

Write the formula for strontium nitride. a) Sr3N2 b) Sr(NO3)2 c) SrN d) Sr2N3 e) Sr(NO2)2

A

A sample of milk is found to have arsenic at a concentration of 1.81 µg/L. What is the concentration in ounces per gallon? 1 qt = 946.4 mL 1 gal = 4 qt 16 oz = 1 lb 1 lb = 0.4536 kg a) 1.95 10^-4 oz/gal b) 2.41 10^-7 oz/gal c) 1.25 oz/gal d) 1.68 10^-8 oz/gal e) 1.36 10^3 oz/gal

B

At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion? a. CO and CO2 b. CO and N2 c. NO2 and N2O4 d. N2O and NO2 e. N2 and O2

B

Choose the name-formula pair that does NOT correctly match. a. aluminum phosphate AlPO4 b. calcium acetate CH3COOCa c. ammonium sulfide (NH4)2S d. magnesium hydroxide Mg(OH)2 e. sodium bicarbonate NaHCO3

B

Combustion analysis of an unknown compound containing only carbon and hydrogen produced 0.2845 g of CO2 and 0.1451 g of H2O. What is the empirical formula of the compound? a) CH2 b) C2H5 c) C4H10 d) C5H2 e) C8H20

B

Combustion of 7.54 g of liquid benzene (C6H6) causes a temperature rise of 50.3°C in a constant-pressure calorimeter that has a heat capacity of 6.27 kJ/°C. What is ∆H for the following reaction? C6H6(l) + O2(g) → 6CO2(g) + 3H2O(l) a. -315 kJ/mol b. -3.27 × 103 kJ/mol c. -41.8 kJ/mol d. 315 kJ/mol e. 41.8 kJ/mol

B

How many aluminum atoms are there in 66 g of Al2S3? a) 2.6 × 10^23 b) 5.3 × 10^23 c) 7.9 × 10^23 d) 1.3 × 10^21 e) 2.0 × 10^21

B

The complete combustion of phenylhydrazine, C6H5NHNH2, with the oxidizer dinitrogen tetraoxide is shown in the following equation: __ C6H5NHNH2 + __ N2O4 → __ CO2 + __ H2O + __ N2 When this equation is balanced, the sum of all the coefficients (using smallest whole numbers) is A) 30. B) 20. C) 25. D) 10. E) 15.

B

A 14.0-gram sample of an unknown gas occupies 11.2 liters at standard temperature and pressure. Which of the following could be the identity of the gas? I. N2 II. CO2 III. CO a. I only b. II only c. I and III only d. II and III only e. I, II, and III

C

An irregularly shaped metal was weighed by the following difference: Watch glass + metal = 56.7813 g Watch glass = 35.4725g The volume of the metal was determined by placing the metal in a graduated cylinder that had water in it and measuring the volume difference: Graduated cylinder + water + metal = 14.15 mL Graduated cylinder + water = 11.25 mL The density of the metal should be reported as: a. 7.3 g/mL b. 7.4 g/mL c. 7.35 g/mL d. 7.348 g/mL e. 7.3479 g/mL

C

Arrange the following ions in order of increasing radius: Mg2+, Br-, Ca2+ a. Ca2+ < Mg2+ < Br- b. Mg2+ < Br- < Ca2+ c. Mg2+ < Ca2+ < Br- d. Br- < Ca2+ < Mg2+ e. Br- < Mg2+ < Ca2+

C

How many 200-mg aspirin tablets can be made from 20.0 kg of aspirin? a) 1000 b) 10,000 c) 100,000 d) 1,000,000 e) 10,000,000

C

The analysis of an organic compound showed that it contained 0.0700 mol of C, 0.175 mol of H, and 0.0350 mol of N. Its molecular mass is 86 amu. How many atoms of carbon are there in the empirical formula for the compound, and how many are in the molecular formula? A) Empirical: two C atoms; molecular: three C atoms B) Empirical: two C atoms; molecular: six C atoms C) Empirical: two C atoms; molecular: four C atoms D) Empirical: five C atoms; molecular: ten C atoms E) Empirical: three C atoms; molecular: three C atoms

C

The average atomic mass of Eu is 151.96 amu. There are only two naturally occurring isotopes of europium, 151Eu with a mass of 151.0 amu and 153Eu with a mass of 153.0 amu. The natural abundance of the 131Eu isotope must be approximately A) 60%. B) 20%. C) 50%. D) 80%. E) 40%.

C

The mass of sulfuric acid in 50.0 mL of a 6.00 M solution is: a. 3.10 g b. 12.0 g c. 29.4 g d. 294 g e. 300. g

C

What is the correct answer to the following calculation? (14.0186 × 0.00458) + (15.0032 × 0.99542) a. 15.0 b. 15.00 c. 14.999 d. 14.9987 e. 14.99869

C

What is the empirical formula of an oxide of nitrogen that contains 63.64% nitrogen by mass? a) NO b) NO2 c) N2O d) N2O3 e) N2O5

C

Which of the following does NOT describe a metal? a. Good conductor of heat b. Good conductor of electricity c. Tends to gain electrons d. Forms ionic compounds with nonmetals e. Found on the left side of the periodic table

C

Which of the following is a molecular element? a) Kr b) Ag c) S d) Mg e) Ti

C

Which of the following pure substances has the highest melting point? a. NCl3 b. OCl2 c. MgCl2 d. LiCl e. CCl4

C

Which of the following represents the change in electronic configuration that is associated with the first ionization energy of strontium? a. [Kr]5s15p1 → [Kr]5s1 + e- b. [Kr]5s2 → [Kr]5s15p1 c. [Kr]5s2 → [Kr]5s1 + e- d. [Kr]5s2 + e- → [Kr]5s25p1 e. [Kr]5s2 + e- → [Kr]5s3

C

Which of the following solutes, dissolved in 1000 g of water, would provide the greatest number of particles? a. 0.030 mol of urea, CO(NH2)2 b. 0.030 mol of ammonium nitrate, NH4NO3 c. 0.030 mol of barium chloride, BaCl2 d. 0.030 mol of acetic acid, CH3COOH e. 0.030 mol of calcium sulfate, CaSO4

C

Which of the following statements are true? a. The principal quantum number (n) describes the shape of an orbital. b. The angular momentum quantum number (l) describes the size and energy associated with an orbital. c. The magnetic quantum number (ml) describes the orientation of the orbital. d. An orbital is the path that an electron follows during its movement in an atom. e. All of the above are true.

C

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed. a. Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) b. Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) c. 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) d. 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) e. No reaction occurs.

D

How many atoms are present in 123 g of magnesium cyanide? A) 5.65 x 10^27 B) 2.91 x 10^24 C) 2.83 x 10^28 D) 4.85 x 10^24 E) 9.7 x 10^23

D

How many chloride ions are there in 4.50 mol of aluminum chloride? a) 3.00 chloride ions b) 13.5 chloride ions c) 2.71 × 1024 chloride ions d) 8.13 × 1024 chloride ions e) 81.3 × 1024 chloride ions

D

If the electron could have a third spin state (that is, ½, -½, and 0), what would be the ground-state electron configuration of carbon? a. 1s^22s^22p^2 b. 1s^32s^22p^1 c. 1s^22s^4 d. 1s^32s^3 e. 1s^22s^32p^1

D

If the temperature is 178°F, what is the temperature in degrees celsius? a) 352°C b) 451°C c) 67°C d) 81.1°C e) 378°C

D

In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C. a. 0.0975 L b. 1.30 L c. 1.33 L d. 1.36 L e. 1.50 L

D

The behavior of PH3(g) is most likely to approach ideal behavior at: a. 1.0 atm and 100°C. b. 0.10 atm and -100°C. c. 10 atm and 100°C. d. 0.10 atm and 100°C. e. 1.0 atm and 0°C.

D

The melting point of a solid is 39°F. This corresponds to A) 295 K. B) 312 K. C) 286 K. D) 277 K. E) 312 K.

D

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42°C is __________ mmHg. a. 116 b. 395 c. 134 d. 263 e. 0.347

D

What is the best answer to report for the following calculation: [(9.149 g + 8.846 g )/4.06 mL] + 0.302 g/mL? a) 4.73427 g/mL b) 4.7343 g/mL c) 4.734 g/mL d) 4.73 g/mL e) 4.7 g/mL

D

What is the formula for the chloride of praseodymium(III)? A) Pr2(ClO2)3 B) Pr(ClO4)2 C) Pr3Cl D) PrCl3 E) Pr(ClO3)3

D

What volume of methane gas, CH4, has the same number of atoms as 6.00 L of krypton gas at the same temperature and pressure? a. 36.0 L b. 1.00 L c. 6.00 L d. 1.20 L e. 30.0 L

D

When C3H8O(g) reacts with oxygen, what is the sum of ALL of the coefficients in the balanced chemical equation? a. 4 b. 9 c. 23 d. 25 e. None of the above

D

When the equation __ (CH3)2NNH2 + __ N2O4 → __ N2 + __ H2O + __ CO2 is balanced, the sum of all the coefficients (simplest whole number) is: a) 9 b) 10 c) 11 d) 12 e) 13

D

Which of the following elements has chemical properties similar to tellurium (Te)? a) fluorine b) hydrogen c) nitrogen d) sulfur e) magnesium

D

Which of the following is an atomic element? A. Cl B. H C. O D. K E. N

D

Which of the following is/are correct postulates of Bohr's theory of the hydrogen atom? 1. The energy of an electron in an atom is quantized (i.e. only specific energy values are possible). 2. The principal quantum number (n), specifies each unique energy level. 3. An electron transition from a lower energy level to a higher energy level results in an emission of a photon of light. a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1, 2, and 3

D

Which of the following is/are true about electromagnetic radiation? 1. Wavelength is inversely proportional to frequency. 2. Frequency has units of s-1 or Hz. 3. Waves of different wavelengths travel at different speeds in a vacuum. a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1, 2, and 3

D

Which of the following statements concerning water, H2O, is/are true? (i) H2O is a chemical compound. (ii) H2O is a homogeneous mixture of hydrogen and oxygen. (iii) The percentage of hydrogen in H 2O is independent of where the water is obtained. a) (i) only b) (ii) only c) (iii) only d) (i) and (iii) e) (i), (ii) and (iii)

D

Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H2(g) + ½O2(g) → H2O(l); ∆H = -285.8 kJ a. If the equation is multiplied by 2, ∆H becomes -571.6 kJ b. If the equation is reversed, ∆H becomes +285.8 kJ c. Per mole of O2, the change in enthalpy is -571.6 kJ d. The value -571.6 kJ pertains to 1 mol of liquid water e. For the reaction H2(g) + ½O2(g) → H2O(g), ∆H is not equal to -285.8 kJ

D

A 24.1-g mixture of nitrogen and carbon dioxide is found to occupy a volume of 15.1 L when measured at 870.2 mmHg and 31.2°C. What is the mole fraction of nitrogen in this mixture? a. 0.539 b. 0.500 c. 0.461 d. 0.426 e. 0.574

E

A 75.0 g sample of pure liquid, liquid A, with a density of 3.00 g/mL is mixed with a 50.0-mL sample of a pure liquid, liquid B, with a density of 2.00 g/mL. What is the total volume of the mixture? (Assume there is no reaction upon mixing of A and B.) a) 275 mL b) 175 mL c) 125 mL d) 100. mL e) 75 mL

E

According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g) a. 28.33 g b. 14.00 g c. 8.33 g d. 19.78 g e. 17.22 g

E

All of the following have a standard enthalpy of formation value of zero at 25°C except: a. C(s) b. Ne(g) c. Fe(s) d. F2(g) e. CO(g)

E

Analysis of a compound containing only C and Br revealed that it contains 33.33 % C atoms by number and has a molar mass of 515.46 g/mol. What is the molecular formula of this compound? A) CBr2 B) C2Br6 C) C2Br4 D) CBr3 E) C3Br6

E

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy? a. 2s → 3p b. 2p → 6d c. 6p → 4s d. 7f → 5d e. 3p → 2s

E

Give the set of four quantum numbers that could represent the electron lost to form the Rb ion from the neutral Rb atom. a. n = 6, l = 0, ml = 0, ms = -1/2 b. n = 4, l = 1, ml = 1, ms = -1/2 c. n = 5, l = 1, ml = 0, ms = +1/2 d. n = 4, l = 1, ml = 0, ms = -1/2 e. n = 5, l = 0, ml = 0, ms = +1/2

E

How many neutrons are there in the cobalt-59 nuclide? A) 27 B) 2 C) 86 D) 59 E) 32

E

What is (are) the spectator ion(s) in the following reaction? 2 HClO3(aq) + Sr(OH)2(aq) → Sr(ClO3)2(aq) + 2 H2O(l) a. H+, OH- b. Sr2+, OH- c. H+ d. OH- e. Sr2+, ClO3-

E

What is the ratio of oxygen atoms to hydrogen atoms in the mineral carnotite, K2(UO2)3(VO4)2·3H2O a) 8:3 b) 8:6 c) 9:6 d) 17:3 e) 17:6

E

Which of the following elements has chemical properties similar to rubidium (Rb)? a) fluorine b) oxygen c) nitrogen d) sulfur e) sodium

E

Which of the following gases has the greatest density at 2.5 atm and 25°C? a. C3H8 b. SO2 c. N2O d. O2 e. NF3

E

Which of the following orbital occupancy designations is incorrect? A) 3d7 B) 2p6 C) 4f6 D) 1s2 E) 4f15

E

Which of the following samples has the fewest moles of gas? a. 1.00 L of CH4 at 10°C and 1.00 atm b. 1.00 L of Ar at -10.0°C and 1.00 atm c. 1.00 L of NH3 at STP d. 1.00 L of H2 at 0.0°C and 1.56 atm e. 1.00 L of HCl at 30°C and 1.00 atm

E