Ch 10 Class Problem Set

4.6 g to milligrams

4.6 g —(1000 mg/1 g)—> 4600 mg

0.107 g to centigrams

0.107 g —(100cg/1g)—>10.7 cg

15 mL to liters

15 mL —(1 L/1000 mL)—> 0.015 L

42.7 L to mL

42.7 L —(1000 mL/1 L)—> 42700 mL

Name XeF₄

Xenon tetrafluoride

Name Al₂S₃

aluminum sulfide

Name CoO

cobalt (II) oxide

Name CaI₂

calcium iodide

Name SnCl₂

Tin(II) chloride

Name SeO

Selenium(II) oxide

Name IF₅

Iodine pentafluoride

Name ZnCl₂

Zinc chloride

Formula for Magnesium oxide

MgO

Formula for Tin(IV) sulfide

SnS₂

Formula for Silicon tetrachloride

SiCl₄

Formula for Carbon monoxide

CO

Formula for Barium fluoride

BaF₂

Formula for Calcium hydride

CaH₂

Formula for Magnesium phosphide 

Mg₃P₂

Formula for Barium nitride

Ba₃N₂

Name Fe₂(SO₄)₃ 

Iron(III) sulfate

Name NH₄NO₂

ammonium nitrite

Name CoSO₄ 

copper (II) sulfate

Name K₂O

potassium oxide

Name Ba(OH)₂ 

Barium hydroxide

Name Ca₃(PO₄)₂ 

Calcium phosphate

Name CuCO₃ 

Copper(II) carbonate

Name Al(HSO₄)₃

Aluminum hydrogen sulfate

How many moles are equal to 9.03 x 10²⁴ atoms of Hg?

9.03 x 10²⁴ atoms of Hg —(1 mol Hg /6.02 × 10²³ atoms Hg)—> 15.0 mol Hg

Calculate the number of moles in 1.00 x 10² g of sucrose (C₁₂H₂₂O₁₁)

1.00 x 10² g C₁₂H₂₂O₁₁ —( 1 mol C₁₂H₂₂O₁₁/ 342 g C₁₂H₂₂O₁₁)—> 0.292 mol C₁₂H₂₂O₁₁

Calculate the number of moles in 1.00 x 10² g. of sodium chloride

1.00 x 10² g NaCl —(1 mol NaCl/58 g NaCl)—> 1.72 mol NaCl

Calculate the number of moles in 1.00 x 10² g. of potassium permanganate

1.00 x 10² g KMnO₄ —(1 mol KMnO₄/ 158 g KMnO₄)—> 0.633 mol KMnO₄

How many atoms are in 1 mole of sucrose (C₁₂H₂₂O₁₁)?

1 mol C₁₂H₂₂O₁₁ —(6.02 × 10²³ atoms C₁₂H₂₂O₁₁/1 mol C₁₂H₂₂O₁₁)—> 6.02 × 10²³ atoms C₁₂H₂₂O₁₁

Calculate the mass in grams for 0.250 mol of sucrose (C₁₂H₂₂O₁₁)

0.250 mol C₁₂H₂₂O₁₁ —(342 g C₁₂H₂₂O₁₁/1 mol C₁₂H₂₂O₁₁)—> 85.5 g C₁₂H₂₂O₁₁

Calculate the mass in grams for 0.250 mol of sodium chloride

0.250 mol NaCl —(58 g NaCl/1 mol NaCl)—> 14.5 g NaCl

Calculate the mass in grams for 0.250 mol of potassium permanganate

0.250 mol KMnO₄—(158 g KMnO₄/1 mol KMnO₄)— 39.5 g KMnO₄

How many moles are in 4.25 x 10²⁴ molecules of NO₂?

4.25 x 10²⁴ molecules NO₂ —(1 mol NO₂/6.02 × 10²³ molecules NO₂)—> 7.06 mol NO₂

Find the number of moles in 3.70 x 10^-1 g. of boron.

3.70 x 10^-1 g B —(1 mol B/11g B)—> 0.0336 mol B

The density of a gaseous compound containing carbon and oxygen is found to be 1.964 g/L at STP. What is the molar mass of the compound?

1.964 g/L —(22.4 L/ 1 mol)—> 43.99 g/mol

At STP, what is the volume occupied by 6.7 mol of hydrogen gas?

6.7 mol H₂ —(22.4 L H₂/1 mol H₂)—> 150 L H₂

How many moles in 15.5 g. SiO₂

15.5 g SiO₂ —(1 mol SiO₂/60 g SiO₂)—> 0.258 mol SiO₂

How many moles in 79.3 g. Cl₂

79.3 g Cl₂ —(1 mol Cl₂/70 g Cl₂)—> 1.13 mol Cl₂

Mass of 1.50 mol C₅H₁₂

1.50 mol C₅H₁₂ —(72 g C₅H₁₂/1 mol C₅H₁₂)—> 108 g C₅H₁₂

Mass of 0.780 mol Ca(CN)₂

0.780 mol Ca(CN)₂ —(92 g Ca(CN)₂/1 mol Ca(CN)₂)—> 65.1 g Ca(CN)₂

Determine the percent composition for Ag₂O. 

Ag: 2(108)/232 × 100 = 93%

O: 16/232 × 100 = 7%

Determine the percent composition for Na₂O. 

Na: 2(23)/62 × 100 = 74%

O: 16/62 × 100 = 26%

What is the volume of 3.20 x 10^-3 mol of CO₂? 

3.20 x 10^-3 mol CO₂ —(22.4 L CO₂/1 mol CO₂)—> 0.0717 L CO₂

Find the mass of 1.50 mol C₅H₁₂.

1.50 mol C₅H₁₂ —(72 g C₅H₁₂/1 mol C₅H₁₂)—> 108 g C₅H₁₂

How many moles are equal to 9.03 x 10²⁴ atoms of mercury (Hg)?

9.03 x 10²⁴ atoms Hg —(1 mol Hg/6.02 × 10²³ atoms Hg)—> 15.0 mol Hg

How many moles are equal to 2.41 x 10²⁴ formula units of NaCl?

2.41 x 10²⁴ formula units NaCl —(1 mol NaCl/6.02 × 10²³ formula units NaCl)—> 4.00mol NaCl

How many atoms are in 1.14 mol of SO₃?

1.14 mol SO₃ —(6.02 × 10²³ SO₃/ 1 mol SO₃)(4 atoms SO₃/1 SO₃)—> 2.75 × 10²⁴ atoms SO₃

How many atoms are in 1.75 mol CHCl₃?

1.75 mol CHCl₃ —(6.02 × 10²³ atoms CHCl₃/1 mol CHCl₃)(5 atoms CHCl₃/1 CHCl₃)—> 2.75 × 10²⁴ atoms CHCl₃

Mass of one mole of CO₂

1 mol CO₂—(44 g CO₂/1 mol CO₂)—> 44 g CO₂

Mass of one mole of SO₃

1 mol SO₃ —(80 g SO₃/1 mol SO₃)—> 80 g SO₃

Mass of one mole of Br₂

1 mol Br₂ —(160 g Br₂/1 mol Br₂)—> 160 g Br₂

Mass of one mole of H₂

1 mol H₂ —(2 g H₂/1 mol H₂)—> 2 g H₂

Mass of one mole of N₂

1 mol —(28 g N₂/1 mol N₂)—> 28 g N₂

What is the mass, in grams, of 1.72 mol of CaCl₂?

1.72 mol CaCl₂ —(110 g CaCl₂/1 mol CaCl₂)—> 189 g CaCl₂

What is the mass of 9.45 mol of aluminum oxide (Al₂O₃)?

9.45 mol Al₂O₃ —(102 g Al₂O₃/1 mol Al₂O₃)—> 964 g Al₂O₃

How many moles of iron(III) oxide are contained in 92.2 g. of pure iron(III) oxide?

92.2 g Fe₂O₃ —(1 mol Fe₂O₃/ 160 g Fe₂O₃)—> 0.576 mol Fe₂O₃

Sulfur dioxide is a gas produced by burning coal. It is an air pollutant and one of the causes of acid rain. Determine the volume, in liters, of 0.60 mol of sulfur dioxide gas at STP.

0.60 mol SO₂ —(22.4 L SO₂/1 mol SO₂)—> 13 L SO₂

At STP, what is the volume occupied by 1.34 mol of SO₂?

1.34 mol SO₂ —(22.4 L SO₂/1 mol SO₂)—> 30.0 L SO₂

A gas has a density of 0.902 g/L. What is the molar mass of this gas at STP?

0.902 g/L —(22.4 L/1 mol)—>20.2 g/mol

At STP, what is the volume occupied by 2.45 x 10^-3 mol of H₂S?

2.45 x 10^-3 mol H₂S —(22.4 L H₂S/1 mol H₂S)—> 0.0549 L H₂S

What is the density of oxygen gas at STP?

1 O₂ —(32 g O₂/1 mol O₂)(1 mol O₂/22.4 L O₂)—> 1.43 g/L O₂

What is the percent composition of the compound formed when 2.70 g. of aluminum combine oxygen to form 5.10 g. of aluminum oxide?

Al: 2.70/5.10 × 100 = 53%

O: 2.40/5.10 × 100 = 47%

Percent composition of Fe₂O₃

Fe: 2(56)/160 × 100 = 70%

O: 3(16)/160 × 100 = 30%

Percent composition of HgO

Hg: 201/217 × 100 = 93%

O: 16/217 × 100 = 7%

What is the empirical formula of the following compound? 36.1% Ca, 63.9% Cl 

Ca: 36.1 g Ca —(1 mol Ca/40 g Ca)—> 0.90 mol Ca

Cl: 63.9 g Cl —(1 mol Cl/35 g Cl)—> 1.82 mol Cl

Ca_0.9Cl_1.8 / 0.9 = CaCl₂

What is the empirical formula of the following compound? 40.0% C, 6.7% H, 53.3% O

C: 36.1 g C —(1 mol C/12 g C)—> 3.33 mol C

H: 6.7 g H —(1 mol H/1 g H)—> 6.7 mol H

O: 53.3 g O —(1 mol O/16 g O)—> 3.33 mol O

C_3.33H_6.7O_3.33 / 3.33 = CH₂O

What is the molecular formula of a compound with the empirical formula CClN and a molar mass of 184.5 g/mol?

empirical formula = 61 g/mol

184.5/61 = 3

molecular formula = C₃Cl₃N₃

What is the molecular formula of a compound that is 56.6% K, 8.7% C, and 34.7% O?

K: 56.6 g Ca —(1 mol K/39 g K)—> 1.5 mol K

C: 8.7 g C —(1 mol C/12 g C)—> 0.7 mol C

O: 34.7 g O —(1 mol O/16 g O)—> 2.2 mol O

K_1.5C_0.7O_2.2 / 0.7 = K₂CO₃