© 2015 Pearson Education, Inc. Chapter 6 Chemical Composition Laurie LeBlanc Cuyamaca College Clicker Questions.

© 2015 Pearson Education, Inc.

Chapter 6

ChemicalComposition

Laurie LeBlancCuyamaca College

Clicker Questions

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A. 3.01 molB. 1.81 × 1047 molC. 1.00 molD. 0.500 molE. 3.01 × 1023 mol

How many moles of Ca are in 3.01 × 1023 atoms of calcium?

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A. 3.01 molB. 1.81 × 1047 molC. 1.00 molD. 0.500 molE. 3.01 × 1023 mol

How many moles of Ca are in 3.01 × 1023 atoms of calcium?

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A. 1 mol C = 12.01 amu CB. 1 mol C = 12.01 g CC. 1 mol C = 6.022 × 1023 atoms C D. Two of the aboveE. All of the above

Which of the following is correct?

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A. 1 mol C = 12.01 amu CB. 1 mol C = 12.01 g CC. 1 mol C = 6.022 × 1023 atoms C D. Two of the aboveE. All of the above

Which of the following is correct?

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A. 1.000 gB. 6.022 × 1023 gC. 0.01791 g D. 26.00 gE. 55.85 g

What is the mass (g) of 1.000 mol of iron?

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A. 1.000 gB. 6.022 × 1023 gC. 0.01791 g D. 26.00 gE. 55.85 g

What is the mass (g) of 1.000 mol of iron?

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A. 112.12 g/molB. 80.05 g/molC. 66.04 g/molD. 114.00 g/molE. 95.23 g/mol

What is the molar mass of ammonium nitrate?

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A. 112.12 g/molB. 80.05 g/molC. 66.04 g/molD. 114.00 g/molE. 95.23 g/mol

What is the molar mass of ammonium nitrate?

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A. 2.33 molB. 2.33 × 103 molC. 2.33 × 10–3 molD. 8.88 × 104 molE. 88.8 mol

How many moles of Pt are in a 455-mg ring of pure platinum?

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A. 2.33 molB. 2.33 × 103 molC. 2.33 × 10–3 molD. 8.88 × 104 molE. 88.8 mol

How many moles of Pt are in a 455-mg ring of pure platinum?

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A. 4.55 gB. 4.31 × 1045 gC. 1.18 × 10–2 g D. 6.02 × 1023 gE. 48.0 g

What is the mass of 4.55 × 1023 copper atoms?

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A. 4.55 gB. 4.31 × 1045 gC. 1.18 × 10–2 g D. 6.02 × 1023 gE. 48.0 g

What is the mass of 4.55 × 1023 copper atoms?

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A. 3.730 × 10–2 molB. 2.268 × 10–3 molC. 2.268 × 103 molD. 5.672 × 10–3 molE. 1.418 × 10–2 mol

How many moles of formula units are in 5.672 g of iron(III) sulfate?

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A. 3.730 × 10–2 molB. 2.268 × 10–3 molC. 2.268 × 103 molD. 5.672 × 10–3 molE. 1.418 × 10–2 mol

How many moles of formula units are in 5.672 g of iron(III) sulfate?

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How many carbon atoms are in 2.6 μg of graphite (pure carbon)?

A. 1.3 × 1017 atomsB. 1.92 × 1019 atomsC. 2.9 × 1022 atomsD. 1.3 × 1020 atomsE. 6.02 × 1023 atoms

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How many carbon atoms are in 2.6 μg of graphite (pure carbon)?

A. 1.3 × 1017 atomsB. 1.92 × 1019 atomsC. 2.9 × 1022 atomsD. 1.3 × 1020 atomsE. 6.02 × 1023 atoms

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A. 0.27 molB. 0.20 molC. 0.16 molD. 0.56 molE. 2.0 × 102 mol

How many moles of formula units are in 5.6 g of lithium nitride?

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A. 0.27 molB. 0.20 molC. 0.16 molD. 0.56 molE. 2.0 × 102 mol

How many moles of formula units are in 5.6 g of lithium nitride?

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A. 2.45 × 1022 formula unitsB. 1.47 × 1022 formula unitsC. 2.95 × 1022 formula unitsD. 1.47 × 1021 formula unitsE. 6.02 × 1023 formula units

How many formula units are in 2.45 g of chalk (calcium carbonate)?

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A. 2.45 × 1022 formula unitsB. 1.47 × 1022 formula unitsC. 2.95 × 1022 formula unitsD. 1.47 × 1021 formula unitsE. 6.02 × 1023 formula units

How many formula units are in 2.45 g of chalk (calcium carbonate)?

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A. 6.90 mol OB. 3.45 mol OC. 5.75 mol OD. 13.5 mol OE. 17.3 mol O

How many moles of oxygen are in 3.45 mol of diphosphorus pentoxide?

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A. 6.90 mol OB. 3.45 mol OC. 5.75 mol OD. 13.5 mol OE. 17.3 mol O

How many moles of oxygen are in 3.45 mol of diphosphorus pentoxide?

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A. 8.66 gB. 20.1 g C. 17.3 gD. 11.2 gE. 0.541 g

How many grams of oxygen are in 40.1 g of calcium hydroxide?

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A. 8.66 gB. 20.1 g C. 17.3 gD. 11.2 gE. 0.541 g

How many grams of oxygen are in 40.1 g of calcium hydroxide?

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A. 5.67 × 1022 moleculesB. 7.19 × 1022 molecules C. 6.02 × 1023 moleculesD. 5.50 × 1023 moleculesE. 3.31 × 1024 molecules

If the density of ethanol (C2H5OH) is 0.789 g/cm3, how many molecules are there in 5.50 mL of this substance?

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A. 5.67 × 1022 moleculesB. 7.19 × 1022 molecules C. 6.02 × 1023 moleculesD. 5.50 × 1023 moleculesE. 3.31 × 1024 molecules

If the density of ethanol (C2H5OH) is 0.789 g/cm3, how many molecules are there in 5.50 mL of this substance?

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A. 90.70 g B. 0.1765 gC. 5.66 g D. 181.4 gE. 0.353 g

What is the mass of 5.660 mol of dinitrogen tetrahydride?

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A. 90.70 g B. 0.1765 gC. 5.66 g D. 181.4 gE. 0.353 g

What is the mass of 5.660 mol of dinitrogen tetrahydride?

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A. 8.1 × 10–3 molB. 210 molC. 1.29 molD. 1.6 × 10–2 molE. 208 mol

How many moles of molecules are in 1.3 g of liquid bromine?

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A. 8.1 × 10–3 molB. 210 molC. 1.29 molD. 1.6 × 10–2 molE. 208 mol

How many moles of molecules are in 1.3 g of liquid bromine?

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A. 0.457 gB. 4.57 gC. 0.129 gD. 0.137 gE. 0.00759 g

What is the mass of 4.57 × 1021 molecules of ammonia, NH3?

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A. 0.457 gB. 4.57 gC. 0.129 gD. 0.137 gE. 0.00759 g

What is the mass of 4.57 × 1021 molecules of ammonia, NH3?

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A. 2 molB. 0.0878 molC. 0.00878 molD. 1.06 × 1023 molE. 0.176 mol

How many moles of sodium are in 5.29 × 1022 formula units of sodium sulfate?

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A. 2 molB. 0.0878 molC. 0.00878 molD. 1.06 × 1023 molE. 0.176 mol

How many moles of sodium are in 5.29 × 1022 formula units of sodium sulfate?

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A. 1 mol OB. 3 mol O C. 6 mol OD. 9 mol OE. 12 mol O

How many moles of oxygen are in one mole of aluminum carbonate?

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A. 1 mol OB. 3 mol O C. 6 mol OD. 9 mol OE. 12 mol O

How many moles of oxygen are in one mole of aluminum carbonate?

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A. CH1.5O and C2H3O2

B. C3H5O3 and C6H10O6 C. C4H6O4 and C8H12O8

D. C4H6O4 and C2H3O2

E. C2H3O2 and C4H6O4

An unknown compound has a molar mass of 118.10 g/mol. Given the following mass percent composition, calculate the empirical and molecular formulas: 40.7% C, 5.13% H, and 54.2% O.

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A. CH1.5O and C2H3O2

B. C3H5O3 and C6H10O6 C. C4H6O4 and C8H12O8

D. C4H6O4 and C2H3O2

E. C2H3O2 and C4H6O4

An unknown compound has a molar mass of 118.10 g/mol. Given the following mass percent composition, calculate the empirical and molecular formulas: 40.7% C, 5.13% H, and 54.2% O.

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A. 380.3 g/molB. 182.3 g/molC. 342.3 g/molD. 129.0 g/molE. 145.5 g/mol

What is the molar mass of sucrose, C12H22O11?

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A. 380.3 g/molB. 182.3 g/molC. 342.3 g/molD. 129.0 g/molE. 145.5 g/mol

What is the molar mass of sucrose, C12H22O11?

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A. 8.23%B. 16.5%C. 28.9%D. 5.21%E. 49.5%

What is the mass percentage of oxygen in caffeine, C8H10N4O2?

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A. 8.23%B. 16.5%C. 28.9%D. 5.21%E. 49.5%

What is the mass percentage of oxygen in caffeine, C8H10N4O2?

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A. C6H8O6

B. C4H4O4 C. C3H4O3 D. CHOE. CH2O

What is the empirical formula of ascorbic acid, C6H8O6, a compound found in citrus fruits?

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A. C6H8O6

B. C4H4O4 C. C3H4O3 D. CHOE. CH2O

What is the empirical formula of ascorbic acid, C6H8O6, a compound found in citrus fruits?

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A. H2 B. N2 C. O2 D. F2

E. Cl2

Identify the diatomic molecule that has a mass of 33.86 g and contains 0.891 moles of molecules.

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A. H2 B. N2 C. O2 D. F2

E. Cl2

Identify the diatomic molecule that has a mass of 33.86 g and contains 0.891 moles of molecules.

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A. Cr2O7

B. Cr2O4

C. CrOD. CrO1.5

E. Cr2O3

Calculate the empirical formula of a 5.85 g sample of an unknown chromium oxide containing 4.00 g of chromium.

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A. Cr2O7

B. Cr2O4

C. CrOD. CrO1.5

E. Cr2O3

Calculate the empirical formula of a 5.85 g sample of an unknown chromium oxide containing 4.00 g of chromium.

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A. CH B. CH2

C. C2HD. C2H3

E. CH3

What is the empirical formula of a compound that contains 14.5% hydrogen and 85.5% carbon by mass?

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A. CH B. CH2

C. C2HD. C2H3

E. CH3

What is the empirical formula of a compound that contains 14.5% hydrogen and 85.5% carbon by mass?

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A. 6.25%B. 26.08%C. 54%D. 52.12%E. 64.32%

What is the mass percentage of oxygen in glycerol, C3H8O3?

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A. 6.25%B. 26.08%C. 54%D. 52.12%E. 64.32%

What is the mass percentage of oxygen in glycerol, C3H8O3?

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A. CH2OB. C3H6O3

C. C6H12O6

D. C2H4O2

E. None of the above

The empirical formula of a compound is found to be CH2O. If its molar mass is 180.2 g/mol, what is the molecular formula of the compound?

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A. CH2OB. C3H6O3

C. C6H12O6

D. C2H4O2

E. None of the above

The empirical formula of a compound is found to be CH2O. If its molar mass is 180.2 g/mol, what is the molecular formula of the compound?

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A. 7.86 gB. 5.35 gC. 7.863 gD. 0.1624 gE. None of the above

A variety of Freon contains 69.58% chlorine by mass. How many grams of chlorine are contained in 11.3 g of this substance?

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A. 7.86 gB. 5.35 gC. 7.863 gD. 0.1624 gE. None of the above

A variety of Freon contains 69.58% chlorine by mass. How many grams of chlorine are contained in 11.3 g of this substance?

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A. 6.527%B. 13.06%C. 19.60%D. 39.17%E. None of the above

What is the mass percentage of oxygen in potassium chlorate?

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A. 6.527%B. 13.06%C. 19.60%D. 39.17%E. None of the above

What is the mass percentage of oxygen in potassium chlorate?

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A. C9H8O4

B. C3H2OC. C2H2O2

D. C2H2OE. None of the above

A compound is found to contain 60.00% C, 4.48% H, and 35.53% O. What is its empirical formula?

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A. C9H8O4

B. C3H2OC. C2H2O2

D. C2H2OE. None of the above

A compound is found to contain 60.00% C, 4.48% H, and 35.53% O. What is its empirical formula?