73.5 Mol Of P4O10 Contains How Many Moles Of P

Question: 1. How many atoms of each element are in a formula unit of magnesium phosphate?

A. 3 magnesium atoms, 2 phosphorus atoms, 8 oxygen atoms
B. 2 magnesium atoms, 3 phosphorus atoms, 12 oxygen atoms
C. 1 magnesium atom, 1 phosphorus atom, 4 oxygen atoms
D. 2 magnesium atoms, 1 phosphorus atom, 4 oxygen atoms
E. 1 magnesium atom, 2 phosphorus atoms, 8 oxygen atoms
Answer: A
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Question: 2. List the number of atoms of each element in a formula unit of ammonium sulfate.

A. 1 nitrogen atom, 4 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms
B. 1 nitrogen atom, 3 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms
C. 2 nitrogen atoms, 6 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms
D. 2 nitrogen atoms, 8 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms
E. 1 nitrogen atom, 4 hydrogen atoms, 2 sulfur atoms, 8 oxygen atoms
Answer: D
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Question: 3. How many atoms of each element are in a formula unit of aluminum carbonate?

A. 3 aluminum atoms, 2 carbon atoms, 6 oxygen atoms
B. 2 aluminum atoms, 3 carbon atoms, 9 oxygen atoms
C. 1 aluminum atom, 1 carbon atom, 3 oxygen atoms
D. 1 aluminum atom, 2 carbon atoms, 6 oxygen atoms
E. 2 aluminum atoms, 1 carbon atom, 3 oxygen atoms
Answer: B
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Question: 4. Which of the following statements is incorrect?

A. Molecular mass is expressed in atomic mass units
B. Formula mass compares the mass of one formula unit of a substance to the mass of one atom of carbon-12
C. Atomic mass has units of grams per atom
D. Both molecular mass and formula mass use carbon-12 as a reference standard
E. Sodium chloride, an ionic compound, is said to have a formula weight, but not a molecular weight
Answer: C
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Question: 5. Which of the following is the best definition of atomic mass?

A. The average mass of the atoms of an element compared to the mass of an atom of carbon-12 at exactly 12 atomic mass units
B. A property reflecting the quantity of matter in a sample
C. The mass of an atom measured in the SI unit of mass, the kilogram
D. The number of grams in a mole of a substance
E. The mass of the number of carbon atoms in exactly 12 grams of carbon-12
Answer: A
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Question: 6. Calculate the formula mass of aluminum carbonate.

A. 87.0 u
B. 114.0 u
C. 147.0 u
D. 201.0 u
E. 234.0 u
Answer: E
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Question: 7. Calculate the formula mass of magnesium phosphate.

A. 119.28 u
B. 143.59 u
C. 214.25 u
D. 262.87 u
E. 333.53 u
Answer: D
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Question: 8. Calculate the molecular mass of butane, C4H10.

A. 124.13 u
B. 58.12 u
C. 34.10 u
D. 14.03 u
E. 13.02 u
Answer: B
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Question: 9. Which of the following statements is/are correct?
i. One mole of a substance contains as many particles as exactly 12 u of carbon-12
ii. A mole of iodine atoms contains fewer atoms than a mole of bromine atoms
iii. There are 6.02 1023 carbon atoms in 12.0 grams of carbon-12
iv. Because both use carbon-12 as a reference, one mole of a low molecular mass substance contains more particles than one mole of a high molecular masssubstance
v. One mole of a substance contains 6.02 1023 particles of that substance

A. i and iii
B. i and v
C. iii and v
D. ii and iv
E. ii and v
Answer: C
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Question: 10. Which of the following statements is/are correct?
i. A mole of sodium atoms (atomic mass = 23.0 u) contains fewer atoms than a mole of potassium atoms (atomic mass = 39.1 u)
ii. A mole of sodium atoms (atomic mass = 23.0 u) contains more atoms than a mole of potassium atoms (atomic mass = 39.1 u)
iii. In effect, the word mole represents the number 6.02 1023
iv. One mole of a substance contains as many particles as there are atoms in 12 grams of carbon-12
v. One mole of molecular nitrogen contains as many molecules as 24.0 u of carbon-12

A. i and iii
B. ii and iii
C. i and iv
D. iii and iv
E. ii, iii, iv, and v
Answer: D
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Question: 11. How many molecules are in 0.105 mol NH3?

A. 6.32 1022
B. 5.73 1024
C. 1.74 10-25
D. 1.58 10-23
E. 1.79
Answer: A
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Question: 12. How many atoms are in 0.188 mol Na?

A. 3.12 10-25
B. 8.84 10-24
C. 1.13 1023
D. 6.02 1023
E. 3.20 1024
Answer: C
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Question: 13. How many moles are in 6.27 1024 formula units of sodium nitrate?

A. 0.0960
B. 10.4
C. 85.0
D. 3.77 1048
E. 2.65 10-49
Answer: B
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Question: 14. Which of the following statements is/are incorrect?
i. The molar mass of carbon-12 is exactly 12 u
ii. The phrase "molar mass of chlorine" is ambiguous
iii. The molar mass of a substance is the mass in grams of 6.02 1023 particles of that substance
iv. For atoms, molar mass is numerically equal to atomic mass
v. The molar masses of elements are always greater, numerically, than the atomic masses of those elements

A. i only
B. i and ii
C. iii and iv
D. i and v
E. ii and v
Answer: D
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Question: 15. Calculate the molar mass of elemental iodine.
A. 126.9 g/mol
B. 253.8 g/mol
C. 79.9 g/mol
D. 159.8 g/mol
E. Only atomic masses, and not molar masses, can be calculated for elements
Answer: B
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Question: 16. Calculate the molar mass of ammonium sulfide.

A. 68.15 g/mol
B. 82.16 g/mol
C. 49.10 g/mol
D. 50.11 g/mol
E. 66.14 g/mol
Answer: A
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Question: 17. Methane, CH4, is a molecular compound. Which of the following is the correct value and units of the molar mass of methane?

A. 16.04 g/mol
B. 16.04 g/molecule
C. 16.04 u
D. 16.04 u/molecule
E. 16.04 g/atom
Answer: A
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Question: 18. What is the mass of 7.24 1023 formula units of barium oxide?

A. 7.85 10-3 g
B. 1.84 102 g
C. 1.11 1026 g
D. 2.84 1045 g
E. 6.68 1049 g
Answer: B
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Question: 19. Calculate the number of moles in 15.8 grams of aluminum hydroxide.

A. 1232 mol
B. 727 mol
C. 15.8 mol
D. 0.343 mol
E. 0.203 mol
Answer: E
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Question: 20. What is the mass of 0.0490 mole of potassium sulfate?

A. 0.0490 g
B. 3.55 kg
C. 6.62 g
D. 8.54 g
E. 174.3 g
Answer: D
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Question: 21. Calculate the number of atoms in 0.377 grams of Ar.

A. 1.57 10-26
B. 2.50 10-23
C. 5.67 1021
D. 9.08 1024
E. 9.42 10-3
Answer: C
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Question: 22. Calculate the percent composition of aluminum oxide.

A. 47.1% Al, 52.9% O
B. 52.9% Al, 47.1% O
C. 28.3% Al, 71.7% O
D. 71.1% Al, 28.3% O
E. 62.8% Al, 37.2% O
Answer: B
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Question: Calculate the percent nitrogen in ammonium nitrate.

A. 17.5%
B. 21.9%
C. 22.9%
D. 33.3%
E. 35.0%
Answer: E
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Question: 24. Calculate the percentage composition of calcium chlorate.

A. 19.4% Ca, 34. 3% Cl, 46.4% O
B. 32.4% Ca, 28.7% Cl, 38.8% O
C. 49.0% Ca, 21.8% Cl, 29.3% O
D. 32.4% Ca, 67.6% ClO3
E. 49.0% Ca, 51.0% ClO3
Answer: A
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Question: 25. How many grams of oxygen are in 8.50 g of formaldehyde, CH2O?

A. 2.12 g
B. 2.83 g
C. 4.25 g
D. 4.53 g
E. 16.0 g
Answer: D
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Question: 26. How many grams of calcium are in 5.00 g of calcium hydroxide?

A. 0.541 g
B. 2.50 g
C. 2.70 g
D. 3.51 g
E. 40.1 g
Answer: C
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Question: 27. Calculate the mass of silver in a sample of silver sulfide that contains 0.890 g of sulfur.

A. 1.08 g
B. 1.78 g
C. 3.00 g
D. 5.99 g
E. 6.89 g
Answer: D
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Question: 28. Which of the following are empirical formulas?
i. C10H8
ii. CH2
iii. Al2Cl6
iv. NO2
v. Hg2Cl2

A. i only
B. i and ii
C. ii and iv
D. i, ii, and v
E. iii, iv, and v
Answer: C
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Question: 29. From the following, pick those that are empirical formulas.
i. KCl
ii. K2S2O8
iii. K2SO4
iv. K4S2
v. KIO3

A. i and v
B. ii and iv
C. iii and iv
D. iv and v
E. i, iii, and v
Answer: E
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Question: 30. A coolant widely used in automobile engines is 38.7% carbon, 9.7% hydrogen, and 51.6% oxygen. Calculate the empirical formula for the compound.
A. C3HO3
B. C2H3O2
C. C2H3O
D. CH3O
E. CHO
Answer: D
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Question: 31. What is the empirical formula of a compound that contains 80.0% carbon and 20.0% hydrogen by mass?

A. CH3
B. CH2
C. CH
D. C3H
E. C2H3
Answer: A
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Question: 32. Which of the following generally indicates the possibility of a chemical change?

i. Color change
ii. Formation of a solid
iii. Formation of a gas
iv. Absorption or release of heat energy
v. Emission of light energy

A. All
B. All but i
C. All but ii
D. All but iii
E. All but v
Answer: A
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Question: 33. A pot of room temperature water is placed on a stovetop burner. After a couple of minutes, small, odorless, colorless bubbles form and bubble out of the liquid. After a few more minutes, similar, larger bubbles form and bubble out at a faster rate. Which of the following is the best explanation of the observations?

A. No change occurs because the bubbles contain no matter.
B. The smaller bubbles are a result of a physical change, and the larger bubbles are the result of a chemical change.
C. The smaller bubbles are the result of a chemical change, and the larger bubbles are the result of a physical change.
D. Both the smaller and larger bubbles are the result of a physical change.
E. Both the smaller and larger bubbles are the result of a chemical change.
Answer: D
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Question: 34. Which of the following chemical equations are balanced correctly?

i. CaCl2(aq) + 2 KF(aq) CaF2(s) + 2 KCl(aq)
ii. C4H10() + 13 O2(g) 4 CO2(g) + 5 H2O(g)
iii. 2 C5H10O() + 15 O2(g) 10 CO2(g) + 10 H2O()

A. i only
B. i and ii
C. i and iii
D. ii and iii
E. i, ii, and iii
Answer: A
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Question: Which correctly matches state symbols with their meanings?

A. (s) = solid, () = liquid, (g) = gas, (a) = aqueous
B. (s) = solid, () = liquid, (g) = gas, (aq) = aqueous
C. (s) = solid, () = liquid, (ga) = gas, (aq) = aqueous
D. (s) = solid, (i) = liquid, (ga) = gas, (aq) = aqueous
E. (so) = solid, (i) = liquid, (ga) = gas, (aq) = aqueous
Answer: B
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Question: 36. When the equation ___ PCl5 + ___ H2O ___ H3PO4 + ___ HCl is properly balanced, what is the sum of the coefficients?

A. 8 or less
B. 9
C. 10
D. 11
E. 12 or more
Answer: D
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Question: 37. When the equation ___ Ca(OH)2 + ___ H3PO4 ___ Ca3(PO4)2 + ___ H2O is properly balanced, what is the sum of the coefficients?

A. 8 or less
B. 9
C. 10
D. 11
E. 12 or more
Answer: E
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Question: 38. What is the coefficient for O2 when the equation ___ C2H6 + ___ O2 ___ CO2 + ___ H2O is properly balanced?

A. 7
B. 6
C. 5
D. 4
E. 3
Answer: A
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Question: 39. What is the coefficient for Zn when the equation ___ Zn + ___ H3PO4 ___ H2 + ___ Zn3(PO4)2 is properly balanced?

A. 1
B. 2
C. 3
D. 4
E. 6
Answer: C
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Question: 40. What is the coefficient for H2 when the equation ___ Ba + ___ H3AsO4 ___ H2 + ___ Ba3(AsO4)2 is properly balanced? Show all the coefficients in the balanced equation above.

A. 1
B. 3
C. 5
D. 2
E. 6
Answer: B
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Question: 41. Consider the hypothetical chemical reaction represented by the equation 3 A + 2 B A3B2 Which of the following is a correct interpretation of this equation?
i. 3 grams of A react with 2 grams of B to form 1 gram of A3B2
ii. 3 atoms of A react with 2 atoms of B to form 1 molecule of A3B2
iii. 3 moles of A react with 2 moles of B to form 1 mole of A3B2

A. i only
B. ii only
C. iii only
D. ii and iii
E. i, ii, and iii
Answer: D
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Question: 42. Consider the hypothetical chemical reaction represented by the equation A + 2 B 3 C + D Which of the following interpretations of this equation is not correct?

A. 1 kg of A reacts with 2 kg of B to form 3 kg of C and 1 kg of D
B. 1 particle of A reacts with 2 particles of B to form 3 particles of C and 1 particle of D
C. 1 dozen particles of A reacts with 2 dozen particles of B to form 3 dozen particles of C and 1 dozen particles of D
D. 1 mole of particles of A reacts with 2 moles of particles of B to form 3 moles of particles of C and 1 mole of particles of D
E. 1 kilomole of particles of A reacts with 2 kilomoles of particles of B to form 3 kilomoles of particles of C and 1 kilomole of particles of D
Answer: A
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Question: 43. Consider the following particulate-level representation of a chemical equation:

Assume that all spheres represent atoms of A. Which of the following is a correctly balanced equation for this reaction?

A. A 2 A
B. A2 2 A
C. 2 A 2 A
D. A A + A
E. A(s) A(g)
Answer: B
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Question: 44. Calcium reacts with the oxygen in the air, forming calcium oxide. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 3 or less
B. 4
C. 5
D. 6
E. 7 or more
Answer: c
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Question: 45. Calcium combines with bromine to make calcium bromide. Write the balanced chemical equation for this reaction. What is the coefficient for bromine?

A. 1
B. 2
C. 3
D. 4
E. 5
Answer: A
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Question: 46. Ammonia is formed from its elements. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 3 or less
B. 4
C. 5
D. 6
E. 7 or more
Answer: D
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Question: 47. When atomic phosphorous (P) and oxygen are directly combined, P4O10 is produced. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 3 or less
B. 5
C. 7
D. 9
E. 10 or more
Answer: E
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Question: 48. When potassium contacts fluorine gas, potassium fluoride is produced. Write the balanced chemical equation for this reaction. What is the coefficient for potassium fluoride?

A. 1
B. 2
C. 3
D. 4
E. 5
Answer: B
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Question: 49. Lithium combines with oxygen to form lithium oxide. Write the balanced chemical equation for this reaction. What is the coefficient for lithium?

A. 4
B. 3
C. 2
D. 1
E. none of the above
Answer: A
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Question: 50. Hypochlorous acid decomposes into water and dichlorine oxide, Cl2O. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 3 or less
B. 4
C. 5
D. 6
E. 7 or more
Answer: B
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Question: 51. Magnesium is placed into sulfuric acid. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 4 or less
B. 5
C. 6
D. 7
E. 8 or more
Answer: A
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Question: 52. Calcium reacts with hydrobromic acid. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 4 or less
B. 5
C. 6
D. 7
E. 8 or more
Answer: B
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Question: 53. A precipitate forms when magnesium chloride and sodium fluoride solutions are combined. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 6
B. 5
C. 4
D. 9
E. none of the above
Answer: A
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Question: 54. The combination of copper(II) nitrate and ammonium sulfide solutions yields a precipitate. Write the balanced chemical equation for this reaction. What is the coefficient for copper(II) nitrate?

A. 3
B. 1
C. 5
D. 2
E. 4
Answer: B
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Question: 55. Solid magnesium hydroxide is added to hydrochloric acid. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 4
B. 5
C. 6
D. 7
E. 8 or more
Answer: C
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Question: 56. A precipitation reaction occurs when barium chloride solution is poured into a solution of sodium sulfate. Write the balanced chemical equation for this reaction. What is the sum of the coefficients?

A. 8 or more
B. 7
C. 6
D. 5
E. 4
Answer: D
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Question: 57. Silver nitrate and sodium chloride solutions are mixed. How many moles of silver nitrate are needed to completely react with 0.327 mole of sodium chloride?

A. 0.981 mol
B. 0.818 mol
C. 0.654 mol
D. 0.327 mol
E. 0.164 mol
Answer: D
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Question: 58. In the reaction P4 + 5 O2 2 P2O5, how many moles of oxygen are consumed each time 0.500 mole of P2O5 is formed?

A. 0.200 mol
B. 0.500 mol
C. 1.25 mol
D. 2.50 mol
E. 5.00 mol
Answer: C
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Question: 59. How many moles of oxygen are consumed in burning 1.60 moles of benzene, C6H6?

A. 6.00 mol
B. 12.0 mol
C. 15.0 mol
D. 18.0 mol
E. 24.0 mol
Answer: B
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Question: 60. How many moles of bromine will react with 0.0500 mole of C2H2 in the reaction C2H2 + 2 Br2 C2H2Br4?

A. 0.100 mol
B. 0.186 mol
C. 0.0250 mol
D. 0.0500 mol
E. 2.00 mol
Answer: A
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Question: 61. In reacting aluminum carbonate with hydrochloric acid according to the equation Al2(CO3)3 + 6 HCl 2 AlCl3 + 3 H2O + 3 CO2, 57.6 mg of carbon dioxide was formed. What mass of aluminum carbonate reacted to form this amount of carbon dioxide?

A. 10.8 mg
B. 32.5 mg
C. 102 mg
D. 306 mg
E. 919 mg
Answer: C
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Question: 62. In the combustion of natural gas according to the equation CH4 + 2 O2 CO2 + 2 H2O, how many grams of water are formed during the combustion of 0.264 mole of CH4?

A. 0.528 g
B. 2.00 g
C. 2.38 g
D. 4.75 g
E. 9.50 g
Answer: E
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Question: 63. In the complete combustion of C3H8O3, how many moles of carbon dioxide are produced when 23.0 g of C3H8O3 burns?

A. 0.250 mol
B. 0.750 mol
C. 0.0833 mol
D. 3.00 mol
E. 33.0 mol
Answer: B
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Question: 64. In the reaction CaCN2 + 3 H2O CaCO3 + 2 NH3, how many kilograms of NH3 will be produced when 25.0 kg of CaCN2 react with excess water?

A. 10.6 kg
B. 12.9 kg
C. 2.66 kg
D. 5.31 kg
E. 7.56 kg
Answer: A
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Question: 65. Barium chloride was used to precipitate silver chloride from a solution of silver nitrate. What mass of barium chloride had to react if 0.635 g of silver chloride formed?

A. 0.437 g
B. 0.461 g
C. 0.874 g
D. 0.923 g
E. 1.85 g
Answer: B
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Question: 66. PCl5 can be produced by the reaction PCl3 + Cl2 PCl5. What mass of PCl3 must be used to produce 127 g of PCl5 if the percent yield is 84.8%?

A. 71.1 g
B. 83.8 g
C. 98.8 g
D. 108 g
E. 150 g
Answer: C
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Question: 67. A chemical reaction resulted in 1.376 g of product, which represented a 78.5 percent yield for the reaction. What is the theoretical yield?

A. 0.785 g
B. 1.08 g
C. 10.8 g
D. 1.75 g
E. 2.16 g
Answer: D
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Question: 68. The reaction C6H6 + HNO3 C6H5NO2 + H2O has a 73.5 percent yield under certain conditions. If 12.75 g of C6H6 is used, how much C6H5NO2 will be produced?

A. 20.1 g
B. 27.4 g
C. 8.09 g
D. 11.0 g
E. 14.8 g
Answer: E
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Question: 69. In a general chemistry laboratory experiment, a student produces 2.73 g of a compound. She calculates the theoretical yield as 3.40 g. What is the percent yield?

A. 9.28%
B. 80.3%
C. 0.803%
D. 125%
E. 1.25%
Answer: B
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Question: 70. Which of the following best describes a limiting reactant?

A. The reactant that limits the rate (or speed) of a chemical reaction.
B. The reactant that limits the position of equilibrium in a reversible chemical change.
C. A reactant with limited nucleophilic hyperconjugation of its s and p orbitals and therefore limited reactivity.
D. A reactant with limited nucleophilic hyperconjugation of its d orbitals and therefore limited reactivity.
E. The reactant that is completely used up by a reaction.
Answer: E
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Question: 71. In the reaction 2 AgI + HgI2 Ag2HgI4, 2.00 g of AgI and 3.50 g of HgI2 were used. Assuming complete reaction of the limiting reactant, what mass of excess reactant remains?

A. 0.191 g AgI
B. 1.94 g AgI
C. 1.94 g HgI2
D. 1.50 g HgI2
E. 1.56 g HgI2
Answer: E
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Question: 72. Calculate the mass of Na2O that can be produced by the reaction of 4.00 g of sodium and 2.00 g of oxygen in the reaction 4 Na + O2 2 Na2O.

A. 1.94 g
B. 2.00 g
C. 4.50 g
D. 5.39 g
E. 6.00 g
Answer: D
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Question: 73. Cu2HgI4 is prepared according to the equation 2 CuI + HgI2 Cu2HgI4. When 2.00 g of each reactant are used, which one is the limiting reactant?

A. Both reactants are limiting
B. This reaction has no limiting reactant
C. CuI
D. HgI2
E. Cu2HgI4
Answer: D
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Question: 74. If the reaction N2 + 3 H2 2 NH3 is carried out using 1.40 g of N2 and 0.400 g of H2, what mass of excess reactant will remain?

A. 0.200 g N2
B. 1.00 g N2
C. 0.100 g H2
D. 0.300 g H2
E. Both reactants will be completely consumed
Answer: C
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Question: 75. Which of the following statements are false?

i. Gases may be compressed.
ii. Gases expand to fill their containers uniformly.
iii. All gases have high density.
iv. Gases may be mixed.
v. A confined gas exerts constant pressure on the walls of its container uniformly in all directions.

A. ii only
B. iii only
C. v only
D. ii and iii
E. ii and v
Answer: B
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Question: 76. Which of the following statements is true?

A. The actual volume of ideal gas molecules is negligible compared to the space they occupy
B. In an ideal gas, the volume of the molecules is typically as low as 10% of the total container volume
C. The distances between ideal gas molecules are usually about the same as the diameter of the molecules
D. Given that there is no chemical reaction between two gases, the ability to mix the gases in a rigid container of fixed volume depends on the external atmospheric pressure
E. Ideal gas molecules usually touch one another in a small container with low pressure and high temperature
Answer: A
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Question: 77. Which of the following statements is false?

A. Particle motion explains why gases fill their containers
B. When an individual particle in a gaseous sample strikes a container wall, it exerts a force at the point of collision
C. Gases consist of molecular particles moving at any given instant in straight lines
D. Gas pressures depend on the depth to which a container is filled with a gas
E. Gas pressures are independent of external factors such as gravitational forces
Answer: D
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Question: 78. Which of the following statements is false?

A. Gas molecules collide with each other without loss of energy
B. Gas molecules collide with the container walls without loss of energy
C. The pressure of a gas at constant temperature in a sealed container will gradually decrease
D. Because of the relationship between temperature and average molecular speed, the temperature of a gas would drop if energy were lost in collisions
E. Friction does not slow down gas particles and cause them to stop moving
Answer: C
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Question: 79. What is the equivalent of 684 torr in mm Hg?

A. 684 mm Hg
B. 0.900 mm Hg
C. 6.75 mm Hg
D. 46.6 mm Hg
E. 1444 mm Hg
Answer: A
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Question: 80. Which of the following is the best definition of pressure?

A. The energy per unit volume.
B. The product of density and volume.
C. The ratio of density to volume.
D. The ratio of volume to density.
E. The force exerted on a unit area.
Answer: E
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Question: 81. The temperature of a gas is 23°C. What is its temperature in kelvins?

A. -250 K (-2.50 102) K
B. 296 K
C. 73 K
D. 45 K
E. 23 K
Answer: B
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Question: 82. The temperature of a gas is 308 K. What is its temperature in degrees Celsius?

A. 35°C
B. 581°C
C. 276°C
D. 171°C
E. 554°C
Answer: A
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Question: 83. Which of the following correctly expresses Charles's Law?

A. V 1/P
B. V n
C. V 1/n
D. V T
E. V 1/T
Answer: D
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Question: 84. 27.7 L of a gas is cooled at constant pressure from 87˚C to 24˚C. What will the volume be at the lower temperature?

A. 0.0438 L
B. 7.64 L
C. 22.9 L
D. 33.6 L
E. 1.00 102 L
Answer: C
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Question: 85. 0.847 L of a gas is heated from 12˚C to 33˚C at constant pressure. What will the volume be at the higher temperature?

A. 1.10 L
B. 0.909 L
C. 0.789 L
D. 0.308 L
E. 2.33 L
Answer: B
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Question: 86. A container holds 34.3 m3 of gas at 65˚C. If pressure remains constant, what will the volume be if the temperature falls to 25˚C?

A. 38.9 m3
B. 0.0331 m3
C. 89.2 m3
D. 30.2 m3
E. 13.2 m3
Answer: D
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Question: 87. A small container has a flexible wall that allows a fixed quantity of gas to remain at constant pressure as the temperature changes. From a starting point of 57.0 mL at 22˚C, to what volume will the system change if the temperature rises to 35˚C?

A. 0.0168 mL
B. 35.8 mL
C. 54.6 mL
D. 59.5 mL
E. 90.7 mL
Answer: D
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Question: 88. A fixed quantity of a gas is maintained at constant pressure as the volume decreases from 1.75 L to 1.25 L. If the temperature was 57˚C at the larger volume, what is it at the smaller volume?

A. -37˚C
B. 41˚C
C. 80˚C
D. 189˚C
E. 236˚C
Answer: A
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Question: 89. A gas sample was originally in a 2.50 102 mL container at 25˚C. The gas was transferred to an evacuated 5.00 102 mL container, and the pressure was the same in both containers. What is the temperature of the gas in the larger container?

A. 596˚C
B. 323˚C
C. 50˚C
D. 13˚C
E. -124˚C
Answer: B
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Question: 90. Which of the following correctly describes the relationship between the volume and pressure of a fixed quantity of an ideal gas at constant temperature?

i. V P
ii. V 1/P
iii. V = kP
iv. V = k(1/P)

A. iv only
B. i and ii
C. iii and iv
D. i and iii
E. ii and iv
Answer: E
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Question: 91. Which of the following correctly expresses Boyle's Law?

A. V 1/P
B. V P
C. V n
D. V 1/T
E. V T
Answer: A
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Question: 92. The pressure on 474 mL of a gas is changed from 726 mm Hg to 622 mm Hg. What is the volume at the new pressure?

A. 2.14 108 mL
B. 553 mL
C. 406 mL
D. 0.00246 mL
E. 0.00181 mL
Answer: B
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Question: 93. A balloon is filled with a gas and has a volume of 1.79 L at 2.82 atm pressure. What will its volume be if the pressure is changed to 5.30 atm?

A. 3.36 L
B. 1.05 L
C. 0.952 L
D. 0.297 L
E. 26.8 L
Answer: C
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Question: 94. A cylindrical gas chamber has a piston at one end that can be used to compress or expand the gas. If the gas is initially at 992 torr when the volume is 2.77 L, what will be the volume if the pressure is reduced to 501 torr?

A. 0.182 L
B. 0.715 L
C. 1.40 L
D. 5.48 L
E. 1.38 106 L
Answer: D
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Question: 95. 10.7 L of a gas at 1.75 atm are expanded to 20.0 L at a constant temperature. What is the new gas pressure?

A. 0.0306 atm
B. 0.936 atm
C. 1.07 atm
D. 3.27 atm
E. 375 atm
Answer: B
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Question: 96. The pressure of a gas is 817 torr at 55˚C. The quantity of the gas is fixed and the volume remains constant as the pressure is adjusted to 6.00 102 torr. What is the resulting temperature of the gas?

A. -32˚C
B. 40˚C
C. 174˚C
D. 241˚C
E. 447˚C
Answer: A
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Question: 97. A gas is collected in a container of fixed volume at 25˚C. If the gas exerts a pressure of 685 mm Hg at this temperature, what will the temperature of the gas be when the pressure is 7.60 102 mm Hg?

A. 331˚C
B. 58˚C
C. 28˚C
D. 23˚C
E. -4˚C
Answer: B
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Question: 98. A gas occupies 4.71 liters at 62˚C and 795 torr. What volume will it occupy if it is cooled to 17˚C and compressed to 911 torr?

A. 3.56 L
B. 6.23 L
C. 1.13 L
D. 4.75 L
E. 4.67 L
Answer: A
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Question: 99. Calculate the original volume of a sealed balloon if it was originally at 25˚C and 1.02 atm, and then it was changed to 5.79 L, 77˚C, and 1.72 atm.

A. 4.03 L
B. 3.17 L
C. 8.31 L
D. 2.92 L
E. 11.5 L
Answer: C
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Question: 100. 4.27 L of a gas are collected at 53˚C and 527 torr. What would this volume be if adjusted to STP?

A. 0 L
B. 7.35 L
C. 5.16 L
D. 3.54 L
E. 2.48 L
Answer: E
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