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Which of the following statements is/are correct?


A) Because it is the standard,carbon has a molar mass of exactly one gram per mole
B) The phrase "molar mass of iodine" is not ambiguous,but the phrase "molar mass of potassium" is ambiguous
C) The molar mass of a substance is the mass in grams of one mole of the substance
D) The formula masses of ionic compounds are always larger,numerically,than the molar masses of those compounds
E) None of the above is correct

F) A) and B)
G) A) and C)

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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 mass substance (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

F) A) and D)
G) A) and C)

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Calculate the percent mercury and nitrogen in mercury(II) cyanide.The formula of the cyanide ion is CN-.


A) 20.0% Hg,40.0% N
B) 79.4% Hg,6.2% N
C) 79.4% Hg,11.1% N
D) 83.4% Hg,11.6% N
E) 88.5% Hg,6.2% N

F) B) and E)
G) None of the above

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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

F) A) and C)
G) A) and B)

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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

F) A) and C)
G) A) and E)

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A compound is analyzed and found to contain 0.279 g C,0.0469 g H,and 0.124 g O.Its molecular mass is 116 g/mol.What is its molecular formula?


A) C5H8O3
B) C3H6O
C) C6H12O2
D) CH6O2
E) C2H12O4

F) C) and E)
G) A) and E)

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Consider the following molecule.The identity of the atoms are shown. Consider the following molecule.The identity of the atoms are shown. What is the molar mass of this substance? A) 22.00 g/mol B) 56.02 g/mol C) 28.01 g/mol D) 76.01 g/mol E) 44.01 g/mol What is the molar mass of this substance?


A) 22.00 g/mol
B) 56.02 g/mol
C) 28.01 g/mol
D) 76.01 g/mol
E) 44.01 g/mol

F) B) and E)
G) B) and D)

Correct Answer

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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

F) A) and E)
G) A) and D)

Correct Answer

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Which of the following statements is/are incorrect?


A) One mole is that amount of any substance that contains the same number of units as the number of atoms in exactly 12 grams of carbon-12
B) To three significant figures,there are 6.02 * 1023 units per mole
C) The number of particles in a mole is called Avogadro's number
D) The mass of 1/12 mole of carbon-12 is 1 gram
E) The mole is a fundamental constant derived from the laws of nature

F) A) and B)
G) B) and D)

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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

F) B) and D)
G) None of the above

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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

F) All of the above
G) A) and B)

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Consider the following laboratory chemical. Consider the following laboratory chemical. What is the molecular mass of this substance? A) 31.02 u B) 63.02 u C) 47.02 u D) 126.04 u E) 110.01 u What is the molecular mass of this substance?


A) 31.02 u
B) 63.02 u
C) 47.02 u
D) 126.04 u
E) 110.01 u

F) B) and D)
G) C) and D)

Correct Answer

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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

F) B) and D)
G) C) and D)

Correct Answer

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A compound analyzes as 18.0% carbon,2.26% hydrogen,and 79.7% chlorine.Calculate the empirical formula of the compound.


A) C4H3Cl4
B) C3H2Cl2
C) C3H3Cl2
D) C2H2Cl3
E) C2H3Cl3

F) A) and B)
G) B) and D)

Correct Answer

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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

F) All of the above
G) A) and B)

Correct Answer

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Calculate the percent nitrogen in ammonium nitrate.


A) 17.5%
B) 21.9%
C) 22.9%
D) 33.3%
E) 35.0%

F) C) and E)
G) A) and C)

Correct Answer

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A researcher finds that a compound is composed of 43.6% phosphorus and 56.4% oxygen.In a separate analysis,she finds that it has a molar mass of 142 g/mol.What is the molecular formula of the compound?


A) P4O10
B) P3O7
C) PO2
D) PO
E) P2O5

F) C) and E)
G) A) and B)

Correct Answer

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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

F) A) and B)
G) None of the above

Correct Answer

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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

F) A) and D)
G) A) and C)

Correct Answer

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Determine the molecular formula of a compound that has a molar mass of 264 g/mol and the empirical formula C3H4O3.


A) CHO
B) CH1.33O
C) C9H12O9
D) C6H8O6
E) C3H4O3

F) B) and C)
G) A) and E)

Correct Answer

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