CHEM Openstax Chemistry Chapter 3

An experiment requires 15.0 mL of a 0.100 M solution of HCl. If you have a 12.0 M HCl stock solution in the laboratory, how would you prepare enough 0.1 M solution to run at least 3 experiments? (Outcome # 5) (DOK 3)

A) add 0.833 mL 12 M HCl stock solution to 99.167 mL water

B) add 0.833 mL 12 M HCl stock solution to 49.167 mL water

C) add 0.833 mL 12 M HCl stock solution to 199.167 mL water

add 0.833 mL 12 M HCl stock solution to 99.167 mL water

Which of the following compounds contains the largest number of atoms? (Outcome # 1,2) DOK 2

A) 1.00 mole of NH3

B) 1.00 mole of H2SO4

C) A. 1.00 mole of HBr

1.00 mole of H2SO4

What is the molar mass of (NH4)3PO4? (Outcome # 1,2) DOK 2

A) 113 g

B) 124 g

C) 149 g

149 g

What is the mass in grams of 6.022 x 10^23 molecules of CO2? (Outcome # 1,2) DOK 3

A) 22 g

B) 44 g

C) 66 g

44 g

What is the total number of atoms contained in 2.00 moles of iron? (Outcome # 1,2) DOK 2

A) 118

B) 6.02 x 10^23

C) 1.2 x 10^24

1.2 x 10^24

What is the molar mass of K2CO3? (Outcome # 1,2) DOK 2

A) 138 g/mol

B) 106 g/mol

C) 99 g/mol

138 g/mol

What is the total number of atoms contained in 1.00 mole of sodium? (Outcome # 1,2,9) DOK 2

A) 118

B) 6.02 x 10^23

C) 1.2 x 10^24

6.02 x 10^23

If a hazardous bottle is labeled 20.2 percent by mass Hydrochloric Acid, HCl, with a density of 1.096 g/mL, calculate the molarity of the HCl solution. (Outcome # 1,2,5,8,9,10) (DOK 3)

A) 6.07 M

B) 0.22 M

C) 14.7 M

6.07 M

1. To dilute a HCl solution from 0.500 M to 0.100 M the final volume must be: (Outcome # 1,2,4,5,8) DOK 2

A) 1/5 the original volume

B) 5 times the original volume

C) 50 L

5 times the original volume

How would you prepare a 1 M solution of sodium hydroxide? (Outcome # 5) (DOK 3)

A) add 40.0 grams of sodium hydroxide to 1 L of water

B) add 40.0 grams of sodium hydroxide to 100 L of water

C) add 40.0 grams of sodium hydroxide to 10 L of water

add 40.0 grams of sodium hydroxide to 1 L of water

How would you prepare a 0.5 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) (Paired item 1)

A) add 40.0 grams of sodium hydroxide to 1 L of water

B) add 20.0 grams of sodium hydroxide to 1 L of water

C) add 20.0 grams of sodium hydroxide to 10 L of water

add 20.0 grams of sodium hydroxide to 1 L of water

What is the mass in grams of 1.59 moles of aluminum oxide? (Outcome # 2) (DOK 2)

A) 162 g

B) 0.0156 g

C) 64.1 g

162 g

What is the mass in grams of 0.852 moles of ferric oxide? (Outcome # 2) (DOK 3) (Paired item 1)

A) 5.34 x 10-3 g

B) 187 g

C) 136 g

136 g

How many moles are in 1.77 kg of cuprous sulfate? (Outcome # 2) (DOK 3)

A) 7.93 x 10-3 moles

B) 7.93 moles

C) 395 moles

7.93 moles

How many grams are in 2.05 x 1023 molecules of dinitrogen pentoxide? (Outcome # 2) (DOK 3)

A) 317 g

B) 36.8 g

C) 0.00315 g

36.8 g

How many grams are in 1.02 x 1022 molecules of nitric acid? (Outcome # 2) (DOK 3) (Paired item 1)

A) 1.07 g

B) 3720 g

C) 2.69 x 10-4 g

1.07 g

What is the total number of atoms contained in 2.11 moles of nickel? (Outcome # 2) (DOK 2)

A) 2.85 x 10^23 atoms

B) 1.27 x 10^24 atoms

C) 3.50 x 10-24 atoms

1.27 x 10^24 atoms

How many atoms are in 1.00 mole of Au? (Outcome # 2) (DOK 2) (Paired item 1)

A) 6.02 x 10^23 atoms

B) 1.66 x 10-24 atoms

C) 197 atoms

6.02 x 10^23 atoms

A 44.8 g rhodium sample contains how many rhodium atoms? (Outcome # 2) (DOK 3)

A) 2.62 x 10^23 atoms

B) 6.02 x 10^23 atoms

C) 2.70 x 10^25 atoms

2.62 x 10^23 atoms

What is the molar mass of potassium nitrate? (Outcome # 2) (DOK 2)

A) 85.10 g/mol

B) 140.20 g/mol

C) 101.10 g/mol

101.10 g/mol

Commercial grade fuming nitric acid contains about 90% HNO3 by mass with a density of 1.50 g/mL, calculate the molarity of the HNO3 solution. (Outcome # 9) (DOK 3)

A) 0.214 M

B) 21.4 M

C) 2.14 M

21.4 M

Which of the following is a method used to allow scientists to determine an empirical formula and identify an organic compound by combusting a sample and the resulting combustion products are quantitatively analyzed? (Outcome # 7) (DOK 1)

A) gravimetric analysis

B) combustion analysis

C) thermal analysis

combustion analysis

A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO2 and 5.40 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3)

A) CH3

B) CH

C) CH2

CH3

A 0.125 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 0.4225 g of CO2 and 0.0865 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) (Paired item 1)

A) CH3

B) CH

C) CH2

CH

An unknown organic compound (0.315 g) containing only C, H, and O produces 0.771 of CO2 and 0.105 g of H2O when it undergoes complete combustion. The approximate molar mass is 108 g/mol. Which of the following compounds could be the identification of the unknown? (Outcome # 7) (DOK 3)

A) para-Cresol, CH3C6H4(OH)

B) Benzyl alcohol, C6H5CH2OH

C) 1,2-Benzoquinone, C6H4O2

1,2-Benzoquinone, C6H4O2

Which of the following is an experimental technique used to determine the mass percent of elements found in a compound? (Outcome # 7) (DOK 1)

A) gravimetric analysis

B) mass analysis

C) elemental analysis

elemental analysis

An unknown hydrocarbon compound was analyzed for hydrogen by elemental analysis and results show that it contains 15.88 % H. What is the empirical formula? (Outcome # 7) (DOK 2)

A) C4H9

B) C8H18

C) C12H27

C4H9

A 5.91 g unknown sample analyzed by elemental analysis revealed a composition of 37.51 % C. In addition, it was determined that the sample contains 1.4830 x 10^23 hydrogen atoms and 1.2966 x 10^23 oxygen atoms. What is the empirical formula? (Outcome # 7) (DOK 3)

A) C6H8O7

B) C5H6O3

C) C8H16O5

C6H8O7

What is the concentration in ppm of a 3.7 L solution (d = 1.00 g/mL) containing 4.21 x 10-7 kg of the pesticide DDT? (Outcome # 8) (DOK 2)

A) 1.14 x 10-1 ppm*

B) 1.14 x 10^2 ppm

C) 1.14 x 10^1 ppm

1.14 x 10-1 ppm

When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1)

A) (aq)

B) (l)

C) (s)

(aq)

How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1)

A) (s)

B) (g)

C) (l)

(s)

1. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1)

A) (s)

B) (g)

C) (l)

(l)

How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1)

A) (s)

B) (g)

C) (l)

(g)

What are the proper units for molar mass in chemistry? (Outcome # 6) (DOK 1)

A) amu

B) g/mol

C) g/mmol

g/mol

How many atoms can be found in a mole of mercury? (Outcome # 2) (DOK 2)

A) 201 atoms

B) 6.02 x 10^23 atoms

C) 1.21 x 10^26 atoms

6.02 x 10^23 atoms

A 21.8 g sample of water contains how many water molecules? (Outcome # 2) (DOK 3)

A) 7.29 x 10^23 molecules

B) 6.02 x 10^23 molecules

C) 2.01 x 10-24 molecules

7.29 x 10^23 molecules

A sample has a molar mass of 143 g/mol, identify the sample. (Outcome # 2) (DOK 1)

A) AuCl

B) AcCl

C) AgCl

AgCl

What is the molar mass of 2.50 g of an unknown sample dissolved in 130. mL of water with a concentration of 0.480 M? (Outcome # 4) (DOK 3)

A) 0.062 g/mol

B) 8.65 g/mol

C) 40.1 g/mol

40.1 g/mol

2.50 g of an unknown base is dissolved in 289 mL of water and has a concentration of 0.216 M. What is the identification of the unknown base? (Outcome # 4) (DOK 3)

A) NaOH

B) LiOH

C) KOH

NaOH

How many grams of Hydrogen are present in three moles of Hydrogen? (Outcome # 1,5,9) (DOK 1)

A) two grams

B) six grams

C) one gram

six grams

Which of the following compounds contains the largest number of atoms? (Outcome # 1,9) (DOK 2)

A) 1.00 mole of NH3

B) 1.00 mole of H2SO4

C) 1.00 mole of HBr

1.00 mole of H2SO4

How many atoms are in 12.8 g of copper metal? (Outcome # 6) (DOK 2)

A) 7.71 x 10^24 atoms

B) 1.21 x 10^23 atoms

C) 3.34 x 10-25 atoms

1.21 x 10^23 atoms

How many grams contain 1.45 x 10^21 zinc atoms? (Outcome # 6) (DOK 2)

A) 1.57 x 10-1 g

B) 5.71 x 10^46 g

C) 2.41 x 10-3 g

1.57 x 10-1 g

How many moles are in 11.0 g of silver metal? (Outcome # 6) (DOK 1)

A) 9.81 moles

B) 1.19 x 10^3 moles

C) 1.02 x 10-1 moles

1.02 x 10-1 moles

What is Avogadro's number? (Outcome # 6) (DOK 1)

A) 6.022 x 10^23 particles/mole

B) 6.022 x 10^22 particles/mole

C) 6.022 x 10^24 particles/mole

6.022 x 10^23 particles/mole

Which of the following 85.0 g samples contain the greatest number of atoms? (Outcome # 6) (DOK 3)

A) zinc

B) gold

C) zirconium

zinc

Which of the following 49.5 g samples contain the fewest number of atoms? (Outcome # 6) (DOK 3) (Paired item 1)

A) lead

B) platinum

C) iron

lead

How many atoms are in 1 mole of calcium? (Outcome # 6) (DOK 1)

A) 6.022 x 10^23 atoms

B) 6.022 x 10-23 atoms

C) 6.022 x 10^22 atoms

6.022 x 10^23 atoms

How many moles contain 6.022 x 10^23 lithium atoms? (Outcome # 6) (DOK 1)

A) 6.022 x 10^23 moles

B) 1 mole

C) 2 moles

1 mole