Laurie LeBlanc Cuyamaca College Clicker Questions Chapter 6 Chemical Composition Laurie LeBlanc Cuyamaca College

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

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

Which of the following is correct? 1 mol C = 12.01 amu C 1 mol C = 12.01 g C 1 mol C = 6.022 × 1023 atoms C Two of the above All of the above Answer: D

Which of the following is correct? 1 mol C = 12.01 amu C 1 mol C = 12.01 g C 1 mol C = 6.022 × 1023 atoms C Two of the above All of the above Answer: D

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

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

What is the molar mass of ammonium nitrate? 112.12 g/mol 80.05 g/mol 66.04 g/mol 114.00 g/mol 95.23 g/mol Answer: B

What is the molar mass of ammonium nitrate? 112.12 g/mol 80.05 g/mol 66.04 g/mol 114.00 g/mol 95.23 g/mol Answer: B

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

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

What is the mass of 4.55 × 1023 copper atoms? 4.55 g 4.31 × 1045 g 1.18 × 10–2 g 6.02 × 1023 g 48.0 g Answer: E

What is the mass of 4.55 × 1023 copper atoms? 4.55 g 4.31 × 1045 g 1.18 × 10–2 g 6.02 × 1023 g 48.0 g Answer: E

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

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

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

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

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

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

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

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

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

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

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

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

If the density of ethanol (C2H5OH) is 0 If the density of ethanol (C2H5OH) is 0.789 g/cm3, how many molecules are there in 5.50 mL of this substance? 5.67 × 1022 molecules 7.19 × 1022 molecules 6.02 × 1023 molecules 5.50 × 1023 molecules 3.31 × 1024 molecules Answer: A

If the density of ethanol (C2H5OH) is 0 If the density of ethanol (C2H5OH) is 0.789 g/cm3, how many molecules are there in 5.50 mL of this substance? 5.67 × 1022 molecules 7.19 × 1022 molecules 6.02 × 1023 molecules 5.50 × 1023 molecules 3.31 × 1024 molecules Answer: A

What is the mass of 5.660 mol of dinitrogen tetrahydride? Answer: D

What is the mass of 5.660 mol of dinitrogen tetrahydride? Answer: D

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

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

What is the mass of 4.57 × 1021 molecules of ammonia, NH3? 0.457 g 4.57 g 0.129 g 0.137 g 0.00759 g Answer: C

What is the mass of 4.57 × 1021 molecules of ammonia, NH3? 0.457 g 4.57 g 0.129 g 0.137 g 0.00759 g Answer: C

How many moles of sodium are in 5 How many moles of sodium are in 5.29 × 1022 formula units of sodium sulfate? 2 mol 0.0878 mol 0.00878 mol 1.06 × 1023 mol 0.176 mol Answer: C

How many moles of sodium are in 5 How many moles of sodium are in 5.29 × 1022 formula units of sodium sulfate? 2 mol 0.0878 mol 0.00878 mol 1.06 × 1023 mol 0.176 mol Answer: C

How many moles of oxygen are in one mole of aluminum carbonate? 1 mol O 3 mol O 6 mol O 9 mol O 12 mol O Answer: D

How many moles of oxygen are in one mole of aluminum carbonate? 1 mol O 3 mol O 6 mol O 9 mol O 12 mol O Answer: D

An unknown compound has a molar mass of 118. 10 g/mol 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. CH1.5O and C2H3O2 C3H5O3 and C6H10O6 C4H6O4 and C8H12O8 C4H6O4 and C2H3O2 C2H3O2 and C4H6O4 Answer: E

An unknown compound has a molar mass of 118. 10 g/mol 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. CH1.5O and C2H3O2 C3H5O3 and C6H10O6 C4H6O4 and C8H12O8 C4H6O4 and C2H3O2 C2H3O2 and C4H6O4 Answer: E

What is the molar mass of sucrose, C12H22O11? 380.3 g/mol 182.3 g/mol 342.3 g/mol 129.0 g/mol 145.5 g/mol Answer: C

What is the molar mass of sucrose, C12H22O11? 380.3 g/mol 182.3 g/mol 342.3 g/mol 129.0 g/mol 145.5 g/mol Answer: C

What is the mass percentage of oxygen in caffeine, C8H10N4O2? 8.23% 16.5% 28.9% 5.21% 49.5% Answer: B

What is the mass percentage of oxygen in caffeine, C8H10N4O2? 8.23% 16.5% 28.9% 5.21% 49.5% Answer: B

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

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

Identify the diatomic molecule that has a mass of 33 Identify the diatomic molecule that has a mass of 33.86 g and contains 0.891 moles of molecules. H2 N2 O2 F2 Cl2 Answer: D

Identify the diatomic molecule that has a mass of 33 Identify the diatomic molecule that has a mass of 33.86 g and contains 0.891 moles of molecules. H2 N2 O2 F2 Cl2 Answer: D

Calculate the empirical formula of a 5 Calculate the empirical formula of a 5.85 g sample of an unknown chromium oxide containing 4.00 g of chromium. Cr2O7 Cr2O4 CrO CrO1.5 Cr2O3 Answer: E

Calculate the empirical formula of a 5 Calculate the empirical formula of a 5.85 g sample of an unknown chromium oxide containing 4.00 g of chromium. Cr2O7 Cr2O4 CrO CrO1.5 Cr2O3 Answer: E

What is the empirical formula of a compound that contains 14 What is the empirical formula of a compound that contains 14.5% hydrogen and 85.5% carbon by mass? CH CH2 C2H C2H3 CH3 Answer: B

What is the empirical formula of a compound that contains 14 What is the empirical formula of a compound that contains 14.5% hydrogen and 85.5% carbon by mass? CH CH2 C2H C2H3 CH3 Answer: B

What is the mass percentage of oxygen in glycerol, C3H8O3? 6.25% 26.08% 54% 52.12% 64.32% Answer: D

What is the mass percentage of oxygen in glycerol, C3H8O3? 6.25% 26.08% 54% 52.12% 64.32% Answer: D

The empirical formula of a compound is found to be CH2O 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? CH2O C3H6O3 C6H12O6 C2H4O2 None of the above Answer: C

The empirical formula of a compound is found to be CH2O 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? CH2O C3H6O3 C6H12O6 C2H4O2 None of the above Answer: C

A variety of Freon contains 69. 58% chlorine by mass A variety of Freon contains 69.58% chlorine by mass. How many grams of chlorine are contained in 11.3 g of this substance? 7.86 g 5.35 g 7.863 g 0.1624 g None of the above Answer: A

A variety of Freon contains 69. 58% chlorine by mass A variety of Freon contains 69.58% chlorine by mass. How many grams of chlorine are contained in 11.3 g of this substance? 7.86 g 5.35 g 7.863 g 0.1624 g None of the above Answer: A

What is the mass percentage of oxygen in potassium chlorate? 6.527% 13.06% 19.60% 39.17% None of the above Answer: D

What is the mass percentage of oxygen in potassium chlorate? 6.527% 13.06% 19.60% 39.17% None of the above Answer: D

A compound is found to contain 60. 00% C, 4. 48% H, and 35. 53% O A compound is found to contain 60.00% C, 4.48% H, and 35.53% O. What is its empirical formula? C9H8O4 C3H2O C2H2O2 C2H2O None of the above Answer: A

A compound is found to contain 60. 00% C, 4. 48% H, and 35. 53% O A compound is found to contain 60.00% C, 4.48% H, and 35.53% O. What is its empirical formula? C9H8O4 C3H2O C2H2O2 C2H2O None of the above Answer: A