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Introductory Chemistry

Stephen S. Zumdahl

Chapter 8

Chemical Composition - all with Video Answers

Educators

Chapter Questions

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Problem 1

Merchants usually sell small nuts, washers, and bolts by weight (like jelly beans!) rather than by individually counting the items. Suppose a particular type of washer weighs 0.110 g on the average. What would 100 such washers weigh? How many washers would there be in $100 . \mathrm{g}$ of washers?

PS
Paul Stoner
Numerade Educator
03:03

Problem 2

A particular small laboratory cork weighs $1.63 \mathrm{g}$ whereas a rubber lab stopper of the same size weighs 4.31 g. How many corks would there be in 500. g of such corks? How many rubber stoppers would there be in $500 .$ g of similar stoppers? How many grams of rubber stoppers would be needed to contain the same number of stoppers as there are corks in $1.00 \mathrm{kg}$ of corks?

Angelina Chavez
Angelina Chavez
Numerade Educator
02:12

Problem 3

Define the $a m u$. What is one amu equivalent to in grams?

Shazia Naz
Shazia Naz
Numerade Educator
00:20

Problem 4

Why do we use the average atomic mass of the elements when performing calculations?

Angelina Chavez
Angelina Chavez
Numerade Educator
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Problem 5

Using the average atomic masses for each of the following elements (see the table inside the front cover of this book), calculate the mass, in amu, of each of the following samples.
a. 278 atoms of $\mathrm{Li}$
b. 1 million C atoms
c. $5 \times 10^{25}$ sodium atoms
d. 1 atom of cadmium
e. $6.022 \times 10^{23}$ atoms of mercury

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:01

Problem 6

Using the average atomic masses for each of the following elements (see the table inside the front cover of this book), calculate the number of atoms present in each of the following samples.
a. 52.00 amu of chromium
b. 749.2 amu of arsenic
c. 4274 amu of rubidium
d. 2698 amu of aluminum
e. $1900 .$ amu of fluorine

Vasu Makani
Vasu Makani
Numerade Educator
01:52

Problem 7

What does an average magnesium atom weigh (in amu)? What would 345 magnesium atoms weigh? How many magnesium atoms are contained in a sample of magnesium that has a mass of $2.071 \times$ $10^{4}$ amu?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:10

Problem 8

What does an average iodine atom weigh (in amu)? How many atoms of iodine are contained in a sample of iodine that has a mass of $7.043 \times 10^{4}$ amu? What would 451 iodine atoms weigh?

Lizabeth Tumminello
Lizabeth Tumminello
Numerade Educator
02:15

Problem 9

In 26.98 g of aluminum, there are ______ aluminum atoms present.

Vasu Makani
Vasu Makani
Numerade Educator
02:34

Problem 10

In 78.20 g of potassium, there are ______ potassium atoms present.

Vasu Makani
Vasu Makani
Numerade Educator
04:49

Problem 11

Suppose you have a sample of sodium weighing 11.50 g. How many atoms of sodium are present in the sample? What mass of potassium would you need to have the same number of potassium atoms as there are sodium atoms in the sample of sodium?

Elizaveta Latash
Elizaveta Latash
Numerade Educator
02:02

Problem 12

What mass of iron contains the same number of atoms as $14.01 \mathrm{g}$ of nitrogen?

Vasu Makani
Vasu Makani
Numerade Educator
03:02

Problem 13

What mass of hydrogen contains the same number of atoms as $7.00 \mathrm{g}$ of nitrogen?

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
02:50

Problem 14

What mass of cobalt contains the same number of atoms as $57.0 \mathrm{g}$ of fluorine?

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
02:42

Problem 15

If an average aluminum atom has mass $4.480 \times$ $10^{-23} \mathrm{g},$ what is the average mass of a boron atom in grams?

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
00:48

Problem 16

Calculate the average mass in grams of 1 atom of oxygen.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:43

Problem 17

Which has the smaller mass, 1 mol of He atoms or 4 mol of $\mathrm{H}$ atoms?

Vasu Makani
Vasu Makani
Numerade Educator
01:59

Problem 18

Which weighs more, 0.50 mol of oxygen atoms or 4 mol of hydrogen atoms?

Michelle Stauffer
Michelle Stauffer
Numerade Educator
04:49

Problem 19

Use the average atomic masses given inside the front cover of this book to calculate the number of moles of each element present in each of the following samples.
a. 21.50 g of arsenic
b. $9.105 \mathrm{g}$ of phosphorus
c. $0.05152 \mathrm{g}$ of barium
d. $43.15 \mathrm{g}$ of carbon
e. $26.02 \mathrm{g}$ of chromium
f. $1.951 \mathrm{g}$ of platinum

Vasu Makani
Vasu Makani
Numerade Educator
05:22

Problem 20

Use the average atomic masses given inside the front cover of this book to calculate the number of moles of each element present in each of the following samples.
a. $1.71 \times 10^{-3} \mathrm{g}$ of silver
b. $280.9 \mathrm{mg}$ of silicon
c. $63.45 \mathrm{g}$ of zinc
d. 5.869 g of nickel
e. $128.6 \mathrm{g}$ of uranium
f. 3.251 kg of lithium

Vasu Makani
Vasu Makani
Numerade Educator
04:36

Problem 21

Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples.
a. 0.251 mol of sodium
b. 2.25 mol of helium
c. $4.27 \times 10^{5}$ mol of iron
d. 5.58 mol of copper
e. $1.45 \times 10^{-6}$ mol of lithium
f. 6.25 mol of aluminum

Vasu Makani
Vasu Makani
Numerade Educator
04:23

Problem 22

Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples.
a. $1.76 \times 10^{-3}$ mol of cesium
b. 0.0125 mol of neon
c. $5.29 \times 10^{3}$ mol of lead
d. 0.00000122 mol of sodium
e. 5.51 millimol of arsenic (1 millimol $=1 / 1000$ mol)
f. 8.72 mol of carbon

Vasu Makani
Vasu Makani
Numerade Educator
05:12

Problem 23

Using the average atomic masses given inside the front cover of the text, calculate the number of atoms present in each of the following samples.
a. $1.50 \mathrm{g}$ of silver, $\mathrm{Ag}$
b. 0.0015 mol of copper, $\mathrm{Cu}$
c. $0.0015 \mathrm{g}$ of copper, $\mathrm{Cu}$
d. $2.00 \mathrm{kg}$ of magnesium, $\mathrm{Mg}$
e. 2.34 oz of calcium, $\mathrm{Ca}$
f. $2.34 \mathrm{g}$ of calcium, $\mathrm{Ca}$
g. 2.34 mol of calcium, $\mathrm{Ca}$

Vasu Makani
Vasu Makani
Numerade Educator
05:02

Problem 24

Using the average atomic masses given inside the front cover of the text, calculate the indicated quantities.
a. the number of cobalt atoms in 0.00103 g of cobalt
b. the number of cobalt atoms in 0.00103 mol of cobalt
c. the number of mol of cobalt in $2.75 \mathrm{g}$ of cobalt
d. the number of mol of cobalt represented by $5.99 \times 10^{21}$ cobalt atoms
e. the mass of 4.23 mol of cobalt
f. the number of cobalt atoms in 4.23 mol of cobalt
g. the number of cobalt atoms in $4.23 \mathrm{g}$ of cobalt

David Collins
David Collins
Numerade Educator
00:13

Problem 25

The ______ of a substance is the mass (in grams) of 1 mol of the substance.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:32

Problem 26

The molar mass of a substance can be obtained by ______ the atomic weights of the component atoms.

Vasu Makani
Vasu Makani
Numerade Educator
03:54

Problem 27

Give the name and calculate the molar mass for each of the following substances.
a. $\mathrm{Cr}_{2} \mathrm{O}_{3}$
b. $\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}$
c. $\mathrm{P}_{4} \mathrm{O}_{6}$
d. $\mathrm{Bi}_{2} \mathrm{O}_{3}$
e. $C S_{2}$
f. $\mathrm{H}_{2} \mathrm{SO}_{3}$

Vasu Makani
Vasu Makani
Numerade Educator
03:34

Problem 28

Give the name and calculate the molar mass for each of the following substances.
a. $\mathrm{NO}_{2}$
b. $\mathrm{N}_{2} \mathrm{O}$
c. $\mathrm{XeF}_{4}$
d. NaOCl
e. $\mathrm{HNO}_{3}$
f. $\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$

Vasu Makani
Vasu Makani
Numerade Educator
04:12

Problem 29

Calculate the molar mass for each of the following substances.
a. barium perchlorate
b. magnesium sulfate
c. lead(II) chloride
d. copper(II) nitrate
e. tin(IV) chloride
f. phenol, $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}$

Angelina Chavez
Angelina Chavez
Numerade Educator
03:16

Problem 30

Calculate the molar mass for each of the following substances.
a. ammonium sulfide, $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}$
b. dichlorophenol, $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{OCl}_{2}$
c. barium hydride, $\mathrm{BaH}_{2}$
d. potassium dihydrogen phosphate, $\mathrm{KH}_{2} \mathrm{PO}_{4}$
e. potassium hydrogen phosphate, $\mathrm{K}_{2} \mathrm{HPO}_{4}$
f. potassium phosphate, $\mathrm{K}_{3} \mathrm{PO}_{4}$

Vasu Makani
Vasu Makani
Numerade Educator
08:33

Problem 31

Calculate the number of moles of the indicated substance present in each of the following samples.
a. $21.4 \mathrm{mg}$ of nitrogen dioxide
b. $1.56 \mathrm{g}$ of copper(II) nitrate
c. $2.47 \mathrm{g}$ of carbon disulfide
d. $5.04 \mathrm{g}$ of aluminum sulfate
e. $2.99 \mathrm{g}$ of lead(II) chloride
f. $62.4 \mathrm{g}$ of calcium carbonate

Rashmi Sinha
Rashmi Sinha
Numerade Educator
04:18

Problem 32

Calculate the number of moles of the indicated substance present in each of the following samples.
a. $92.4 \mathrm{g}$ of hydrogen bromide
b. $5.34 \mathrm{mg}$ of ferric chloride
c. $2.21 \mathrm{kg}$ of sulfuric acid
d. $3.44 \mathrm{g}$ of barium carbonate
e. $2.89 \mathrm{g}$ of aluminum chloride
f. $7.21 \mathrm{g}$ of lithium carbonate

Vasu Makani
Vasu Makani
Numerade Educator
03:57

Problem 33

Calculate the number of moles of the indicated substance in each of the following samples.
a. $18.0 \mathrm{g}$ of dextrose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
b. $21.94 \mathrm{g}$ of nitrous oxide, $\mathrm{N}_{2} \mathrm{O}$
c. $21.94 \mathrm{g}$ of nitric oxide, $\mathrm{NO}$
d. 1.24 oz of gold(III) acetate, $\mathrm{Au}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{3}$
e. $44.2 \mathrm{g}$ of ammonium dichromate, $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$

Vasu Makani
Vasu Makani
Numerade Educator
02:38

Problem 34

Calculate the number of moles of the indicated substance in each of the following samples.
a. $4.26 \times 10^{-3} \mathrm{g}$ of sodium dihydrogen phosphate
b. $521 \mathrm{g}$ of copper(I) chloride
c. $151 \mathrm{kg}$ of iron
d. $8.76 \mathrm{g}$ of strontium fluoride
e. $1.26 \times 10^{4} \mathrm{g}$ of aluminum

Angelina Chavez
Angelina Chavez
Numerade Educator
03:25

Problem 35

Calculate the mass in grams of each of the following samples.
a. 2.41 millimol of potassium nitrate (1 millimol $=$ $1 / 1000 \mathrm{mol})$
b. 8.91 mol of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
c. 0.0141 mol of calcium oxide
d. $1.91 \mathrm{mol}$ of gold(III) bromide
e. 0.0000117 mol of water
f. 2.68 mol of silver nitrate

Vasu Makani
Vasu Makani
Numerade Educator
08:56

Problem 36

Calculate the mass in grams of each of the following samples.
a. 0.000471 mol of carbon monoxide
b. $1.75 \times 10^{-6}$ mol of gold(III) chloride
c. 228 mol of iron(III) chloride
d. 2.98 millimol of potassium phosphate (1 millimol = 1/1000 mol)
e. $2.71 \times 10^{-3}$ mol of lithium chloride
f. 6.55 mol of ammonia

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
03:09

Problem 37

Calculate the mass in grams of each of the following samples.
a. 0.251 mol of ethyl alcohol, $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$
b. 1.26 mol of carbon dioxide
c. $9.31 \times 10^{-4}$ mol of gold(III) chloride
d. 7.74 mol of sodium nitrate
e. 0.000357 mol of iron

Vasu Makani
Vasu Makani
Numerade Educator
03:22

Problem 38

Calculate the mass in grams of each of the following samples.
a. 1.27 mmol of carbon dioxide
b. $4.12 \times 10^{3}$ mol of nitrogen trichloride
c. 0.00451 mol of ammonium nitrate
d. 18.0 mol of water
e. 62.7 mol of copper(II) sulfate

Vasu Makani
Vasu Makani
Numerade Educator
08:24

Problem 39

Calculate the number of molecules present in each of the following samples.
a. 4.75 mmol of phosphine, $\mathrm{PH}_{3}$
b. 4.75 g of phosphine, $\mathrm{PH}_{3}$
c. $1.25 \times 10^{-2}$ g of lead(II) acetate, $\mathrm{Pb}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}$
d. $1.25 \times 10^{-2}$ mol of lead(II) acetate, $\operatorname{Pb}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}$
e. a sample of benzene, $\mathrm{C}_{6} \mathrm{H}_{6},$ which contains a total of 5.40 mol of carbon

Shazia Naz
Shazia Naz
Numerade Educator
03:37

Problem 40

Calculate the number of molecules present in each of the following samples.
a. 6.37 mol of carbon monoxide
b. 6.37 g of carbon monoxide
c. $2.62 \times 10^{-6} \mathrm{g}$ of water
d. $2.62 \times 10^{-6}$ mol of water
e. $5.23 \mathrm{g}$ of benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$

Ronald Prasad
Ronald Prasad
Numerade Educator
08:49

Problem 41

Calculate the number of moles of carbon atoms present in each of the following samples.
a. $1.271 \mathrm{g}$ of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
b. $3.982 \mathrm{g}$ of 1,4 -dichlorobenzene, $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$
c. 0.4438 g of carbon suboxide, $\mathrm{C}_{3} \mathrm{O}_{2}$
d. $2.910 \mathrm{g}$ of methylene chloride, $\mathrm{CH}_{2} \mathrm{Cl}_{2}$

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
09:50

Problem 42

Calculate the number of moles of sulfur atoms present in each of the following samples.
a. $2.01 \mathrm{g}$ of sodium sulfate
b. $2.01 \mathrm{g}$ of sodium sulfite
c. $2.01 \mathrm{g}$ of sodium sulfide
d. $2.01 \mathrm{g}$ of sodium thiosulfate, $\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:32

Problem 43

The mass fraction of an element present in a compound can be obtained by comparing the mass of the particular element present in 1 mol of the compound to the ______ mass of the compound.

Lizabeth Tumminello
Lizabeth Tumminello
Numerade Educator
00:28

Problem 44

The mass percentage of a given element in a compound must always be (greater/less) than $100 \%$.

Lizabeth Tumminello
Lizabeth Tumminello
Numerade Educator
02:04

Problem 45

Calculate the percent by mass of each element in the following compounds.
a. $\mathrm{HClO}_{3}$
b. UF $_{4}$
c. $\mathrm{CaH}_{2}$
d. $\mathrm{Ag}_{2} \mathrm{S}$
e. $\mathrm{NaHSO}_{3}$
f. $\mathrm{MnO}_{2}$

David Collins
David Collins
Numerade Educator
04:44

Problem 46

Calculate the percent by mass of each element in the following compounds.
a. $\mathrm{Na}_{2} \mathrm{S}$
b. $\mathrm{NH}_{4} \mathrm{NO}_{2}$
c. $\mathrm{NH}_{4} \mathrm{NO}_{3}$
d. $\mathrm{NH}_{2} \mathrm{Cl}$
e. $\mathrm{PH}_{3}$
f. $\mathrm{H}_{3} \mathrm{PO}_{3}$

Lizabeth Tumminello
Lizabeth Tumminello
Numerade Educator
06:52

Problem 47

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds.
a. methane, $\mathrm{CH}_{4}$
b. sodium nitrate, $\mathrm{NaNO}_{3}$
c. carbon monoxide, $\mathrm{CO}$
d. nitrogen dioxide, $\mathrm{NO}_{2}$
e. 1 -octanol, $\mathrm{C}_{8} \mathrm{H}_{18} \mathrm{O}$
f. calcium phosphate, $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$
g. 3 -phenylphenol, $\mathrm{C}_{12} \mathrm{H}_{10} \mathrm{O}$
h. aluminum acetate, $\mathrm{Al}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{3}$

Cheryl Glor
Cheryl Glor
Numerade Educator
08:13

Problem 48

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds.
a. copper(II) bromide, $\mathrm{CuBr}_{2}$
b. copper(I) bromide, CuBr
c. iron(II) chloride, $\mathrm{FeCl}_{2}$
d. iron(III) chloride, $\mathrm{FeCl}_{3}$
e. cobalt(II) iodide, $\mathrm{Col}_{2}$
f. cobalt(III) iodide, $\mathrm{CoI}_{3}$
g. tin(II) oxide, $\operatorname{SnO}$
h. tin(IV) oxide, $\operatorname{SnO}_{2}$

Abdel Osman
Abdel Osman
Numerade Educator
08:13

Problem 49

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds.
a. adipic acid, $\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O}_{4}$
b. ammonium nitrate, $\mathrm{NH}_{4} \mathrm{NO}_{3}$
c. caffeine, $\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}$
d. chlorine dioxide, $\mathrm{ClO}_{2}$
e. cyclohexanol, $\mathrm{C}_{6} \mathrm{H}_{11} \mathrm{OH}$
f. dextrose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
g. eicosane, $\mathrm{C}_{20} \mathrm{H}_{42}$
h. ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$

Abdel Osman
Abdel Osman
Numerade Educator
07:17

Problem 50

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds.
a. iron(III) chloride
b. oxygen difluoride, $\mathrm{OF}_{2}$
c. benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$
d. ammonium perchlorate, $\mathrm{NH}_{4} \mathrm{ClO}_{4}$
e. silver oxide
f. cobalt(II) chloride
g. dinitrogen tetroxide
h. manganese(II) chloride

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
07:17

Problem 51

For each of the following samples of ionic substances, calculate the number of moles and mass of the positive ions present in each sample.
a. $4.25 \mathrm{g}$ of ammonium iodide, $\mathrm{NH}_{4} \mathrm{I}$
b. 6.31 mol of ammonium sulfide, $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}$
c. $9.71 \mathrm{g}$ of barium phosphide, $\mathrm{Ba}_{3} \mathrm{P}_{2}$
d. 7.63 mol of calcium phosphate, $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$

Ronald Prasad
Ronald Prasad
Numerade Educator
08:16

Problem 52

For each of the following ionic substances, calculate the percentage of the overall molar mass of the compound that is represented by the positive ions the compound contains.
a. ammonium chloride
b. copper(II) sulfate
c. gold(III) chloride
d. silver nitrate

Abdel Osman
Abdel Osman
Numerade Educator
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Problem 53

What experimental evidence about a new compound must be known before its formula can be determined?

FB
Faye Blumberg
Numerade Educator
02:05

Problem 54

What does the empirical formula of a compound represent? How does the molecular formula differ from the empirical formula?

Abdel Osman
Abdel Osman
Numerade Educator
01:27

Problem 55

Give the empirical formula that corresponds to each of the following molecular formulas.
a. sodium peroxide, $\mathrm{Na}_{2} \mathrm{O}_{2}$
b. terephthalic acid, $\mathrm{C}_{8} \mathrm{H}_{6} \mathrm{O}_{4}$
c. phenobarbital, $\mathrm{C}_{12} \mathrm{H}_{12} \mathrm{N}_{2} \mathrm{O}_{3}$
d. 1,4 -dichloro-2-butene, $\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{Cl}_{2}$

Rashmi Sinha
Rashmi Sinha
Numerade Educator
02:12

Problem 56

Which of the following pairs of compounds have the same empirical formula?
a. acetylene, $\mathrm{C}_{2} \mathrm{H}_{2},$ and benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$
b. ethane, $\mathrm{C}_{2} \mathrm{H}_{6},$ and butane, $\mathrm{C}_{4} \mathrm{H}_{10}$
c. nitrogen dioxide, $\mathrm{NO}_{2}$, and dinitrogen tetroxide, $\mathrm{N}_{2} \mathrm{O}_{4}$
d. diphenyl ether, $\mathrm{C}_{12} \mathrm{H}_{10} \mathrm{O},$ and phenol, $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}$

Stephen Ho
Stephen Ho
Numerade Educator
01:47

Problem 57

A compound was analyzed and was found to contain the following percentages by mass: phosphorus, 90.10\%; hydrogen 8.90\%. Determine the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
02:23

Problem 58

A compound was analyzed and was found to contain the following percentages by mass: hydrogen, 3.09\%; phosphorus, 31.60\%; oxygen, 65.31\%. Determine the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
02:48

Problem 59

A 0.5998-g sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.2322 g; hydrogen, 0.05848 g; oxygen, 0.3091 g. Calculate the empirical formula of the compound.

Alexandra Grace
Alexandra Grace
Numerade Educator
02:34

Problem 60

A compound has the following percentages by mass: barium, 58.84\%; sulfur, 13.74\%; oxygen, 27.43\%. Determine the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
02:12

Problem 61

If a $1.271-\mathrm{g}$ sample of aluminum metal is heated in a chlorine gas atmosphere, the mass of aluminum chloride produced is 6.280 g. Calculate the empirical formula of aluminum chloride.

Alexandra Grace
Alexandra Grace
Numerade Educator
03:09

Problem 62

Analysis of a certain compound yielded the following percentages of the elements by mass: nitrogen, 29.16\%; hydrogen, 8.392\%; carbon, 12.50\%; oxygen, 49.95\%. Determine the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
04:37

Problem 63

When $3.269 \mathrm{g}$ of zinc is heated in pure oxygen, the sample gains $0.800 \mathrm{g}$ of oxygen in forming the oxide. Calculate the empirical formula of zinc oxide.

William Talbert
William Talbert
Numerade Educator
02:27

Problem 64

If cobalt metal is mixed with excess sulfur and heated strongly, a sulfide is produced that contains $55.06 \%$ cobalt by mass. Calculate the empirical formula of the sulfide.

Alexandra Grace
Alexandra Grace
Numerade Educator
02:08

Problem 65

If $2.461 \mathrm{g}$ of metallic calcium is heated in a stream of chlorine gas, $4.353 \mathrm{g}$ of $\mathrm{Cl}_{2}$ is absorbed in forming the metal chloride. Calculate the empirical formula of calcium chloride.

Vasu Makani
Vasu Makani
Numerade Educator
02:35

Problem 66

If $10.00 \mathrm{g}$ of copper metal is heated strongly in the air, the sample gains $2.52 \mathrm{g}$ of oxygen in forming an oxide. Determine the empirical formula of this oxide.

Abdel Osman
Abdel Osman
Numerade Educator
02:05

Problem 67

A compound used in the nuclear industry has the following composition: uranium, $67.61 \% ;$ fluorine, 32.39\%. Determine the empirical formula of the compound.

Alexandra Grace
Alexandra Grace
Numerade Educator
02:02

Problem 68

A compound has the following percentages by mass: aluminum, 32.13\%; fluorine, 67.87\%. Calculate the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
02:44

Problem 69

A compound has the following percentage composition by mass: copper, 33.88\%; nitrogen, 14.94\%; oxygen, $51.18 \% .$ Determine the empirical formula of the compound.

Alexandra Grace
Alexandra Grace
Numerade Educator
01:46

Problem 70

When lithium metal is heated strongly in an atmosphere of pure nitrogen, the product contains $59.78 \% \mathrm{Li}$ and $40.22 \% \mathrm{N}$ on a mass basis. Determine the empirical formula of the compound.

Alexandra Grace
Alexandra Grace
Numerade Educator
02:18

Problem 71

A compound has been analyzed and has been found to have the following composition: copper, $66.75 \%$ phosphorus, $10.84 \% ;$ oxygen, $22.41 \% .$ Determine the empirical formula of the compound.

Alexandra Grace
Alexandra Grace
Numerade Educator
02:20

Problem 72

A compound was analyzed and found to have the following percentage composition: aluminum, $15.77 \% ;$ sulfur, $28.11 \% ;$ oxygen, $56.12 \% .$ Calculate the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
02:26

Problem 73

When $1.00 \mathrm{mg}$ of lithium metal is reacted with fluorine gas $\left(\mathrm{F}_{2}\right),$ the resulting fluoride salt has a mass of $3.73 \mathrm{mg}$. Calculate the empirical formula of lithium fluoride.

Alexandra Grace
Alexandra Grace
Numerade Educator
03:47

Problem 74

Phosphorus and chlorine form two binary compounds, in which the percentages of phosphorus are $22.55 \%$ and $14.87 \%,$ respectively. Calculate the $\mathrm{em}-$ pirical formulas of the two binary phosphoruschlorine compounds.

Vasu Makani
Vasu Makani
Numerade Educator
02:09

Problem 75

How does the molecular formula of a compound differ from the empirical formula? Can a compound's empirical and molecular formulas be the same? Explain.

Temi Ajayi
Temi Ajayi
Numerade Educator
05:01

Problem 76

What information do we need to determine the molecular formula of a compound if we know only the empirical formula?

Temi Ajayi
Temi Ajayi
Numerade Educator
07:44

Problem 77

A binary compound of boron and hydrogen has the following percentage composition: $78.14\%$ boron, $21.86 \%$ hydrogen. If the molar mass of the compound is determined by experiment to be between 27 and 28 g, what are the empirical and molecular formulas of the compound?

Temi Ajayi
Temi Ajayi
Numerade Educator
04:56

Problem 78

A compound with empirical formula CH was found by experiment to have a molar mass of approximately 78 g. What is the molecular formula of the compound?

Temi Ajayi
Temi Ajayi
Numerade Educator
04:50

Problem 79

A compound with the empirical formula $\mathrm{CH}_{2}$ was found to have a molar mass of approximately $84 \mathrm{g}$ What is the molecular formula of the compound?

Temi Ajayi
Temi Ajayi
Numerade Educator
01:56

Problem 80

A compound with the empirical formula $\mathrm{CH}_{4} \mathrm{O}$ was found in a subsequent experiment to have a molar mass of approximately $192 \mathrm{g}$. What is the molecular formula of the compound?

Abdel Osman
Abdel Osman
Numerade Educator
03:19

Problem 81

A compound having an approximate molar mass of $165-170$ g has the following percentage composition by mass: carbon, $42.87\%;$ hydrogen, $3.598\%;$ oxygen, $28.55\%;$ nitrogen, $25.00\%.$ Determine the empirical and molecular formulas of the compound.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:57

Problem 82

A very toxic sodium compound consists of $46.91 \%$ $\mathrm{Na}, 24.51 \% \mathrm{C},$ and $28.59 \% \mathrm{N}$ on a mass basis and has a molar mass of approximately $50 \mathrm{g} / \mathrm{mol} .$ Determine the empirical and molecular formulas of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
12:56

Problem 83

Use the periodic table inside the front cover of this text to determine the atomic mass (per mole) or molar mass of each of the substances in column $1,$ and find that mass in column $2.$
$\begin{array}{ll}\text { Column 1 } & \text { Column 2 } \\ \text { (1) molybdenum } & \text { (a) } 33.99 \mathrm{g} \\ \text { (2) lanthanum } & \text { (b) } 79.9 \mathrm{g} \\ \text { (3) carbon tetrabromide } & \text { (c) } 95.94 \mathrm{g} \\ \text { (4) mercury(II) oxide } & \text { (d) } 125.84 \mathrm{g} \\ \text { (5) titanium(IV) oxide } & \text { (e) } 138.9 \mathrm{g} \\ \text { (6) manganese(II) chloride } & \text { (f) } 143.1 \mathrm{g} \\ \text { (7) phosphine, } \mathrm{PH}_{3} & \text { (g) } 156.7 \mathrm{g} \\ \text { (8) tin(II) fluoride } & \text { (h) } 216.6 \mathrm{g} \\ \text { (9) lead(II) sulfide } & \text { (i) } 239.3 \mathrm{g} \\ \text { (10) copper(I) oxide } & \text { (j) } 331.6 \mathrm{g}\end{array}$

Temi Ajayi
Temi Ajayi
Numerade Educator
02:54

Problem 84

Complete the following table.

Bryan Lynn
Bryan Lynn
Numerade Educator
02:54

Problem 85

Complete the following table.

Bryan Lynn
Bryan Lynn
Numerade Educator
06:00

Problem 86

Consider a hypothetical compound composed of elements $\mathrm{X}, \mathrm{Y},$ and $\mathrm{Z}$ with the empirical formula $\mathrm{X}_{2} \mathrm{YZ}_{3} .$ Given that the atomic masses of $\mathrm{X}, \mathrm{Y},$ and $\mathrm{Z}$ are $41.2,57.7,$ and $63.9,$ respectively, calculate the percentage composition by mass of the compound. If the molecular formula of the compound is found by molar mass determination to be actually $\mathrm{X}_{4} \mathrm{Y}_{2} \mathrm{Z}_{6 \prime}$ what is the percentage of each element present? Explain your results.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
10:03

Problem 87

A binary compound of magnesium and nitrogen is analyzed, and $1.2791 \mathrm{g}$ of the compound is found to contain $0.9240 \mathrm{g}$ of magnesium. When a second sample of this compound is treated with water and heated, the nitrogen is driven off as ammonia, leaving a compound that contains $60.31 \%$ magnesium and $39.69 \%$ oxygen by mass. Calculate the empirical formulas of the two magnesium compounds.

Temi Ajayi
Temi Ajayi
Numerade Educator
07:11

Problem 88

When a $2.118-g$ sample of copper is heated in an atmosphere in which the amount of oxygen present is restricted, the sample gains $0.2666 \mathrm{g}$ of oxygen in forming a reddish-brown oxide. However, when 2.118 g of copper is heated in a stream of pure oxygen, the sample gains $0.5332 \mathrm{g}$ of oxygen. Calculate the empirical formulas of the two oxides of copper.

Temi Ajayi
Temi Ajayi
Numerade Educator
07:15

Problem 89

Hydrogen gas reacts with each of the halogen elements to form the hydrogen halides (HF, HCl, HBr, HI). Calculate the percent by mass of hydrogen in each of these compounds.

Temi Ajayi
Temi Ajayi
Numerade Educator
12:13

Problem 90

Calculate the number of atoms of each element present in each of the following samples.
a. 4.21 g of water
b. $6.81 \mathrm{g}$ of carbon dioxide
c. $0.000221 \mathrm{g}$ of benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$
d. $2.26 \mathrm{mol}$ of $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$

Temi Ajayi
Temi Ajayi
Numerade Educator
03:54

Problem 91

Calculate the mass in grams of each of the following samples.
a. 10,000,000,000 nitrogen molecules
b. $2.49 \times 10^{20}$ carbon dioxide molecules
c. 7.0983 mol of sodium chloride
d. $9.012 \times 10^{-6}$ mol of 1,2 -dichloroethane, $\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}$

Chareen Guzman
Chareen Guzman
Numerade Educator
21:54

Problem 92

Calculate the mass of carbon in grams, the percent carbon by mass, and the number of individual carbon atoms present in each of the following samples.
a. 7.819 g of carbon suboxide, $\mathrm{C}_{3} \mathrm{O}_{2}$
b. $1.53 \times 10^{21}$ molecules of carbon monoxide
c. 0.200 mol of phenol, $C_{6} \mathrm{H}_{6} \mathrm{O}$

Temi Ajayi
Temi Ajayi
Numerade Educator
11:44

Problem 93

Find the item in column 2 that best explains or completes the statement or question in column 1.
Column 1
(1) 1 amu
(2) 1008 amu
(3) mass of the "average" atom of an element
(4) number of carbon atoms in $12.01 \mathrm{g}$ of carbon
(5) $6.022 \times 10^{23}$ molecules
(6) total mass of all atoms in 1 mol of a compound
(7) smallest whole-number ratio of atoms present in a molecule
(8) formula showing actual number of atoms present in a molecule
(9) product formed when any carbon-containing compound is burned in $\mathrm{O}_{2}$
(10) have the same empirical formulas, but different molecular formulas
Column 2
(a) $6.022 \times 10^{23}$
(b) atomic mass
(c) mass of 1000 hydrogen atoms
(d) benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$, and acetylene, $\mathrm{C}_{2} \mathrm{H}_{2}$
(e) carbon dioxide
(f) empirical formula
(g) $1.66 \times 10^{-24} \mathrm{g}$
(h) molecular formula
(i) molar mass
(j) 1 mol

Temi Ajayi
Temi Ajayi
Numerade Educator
04:39

Problem 94

Calculate the number of grams of iron that contain the same number of atoms as $2.24 \mathrm{g}$ of cobalt.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
02:48

Problem 95

Calculate the number of grams of cobalt that contain the same number of atoms as $2.24 \mathrm{g}$ of iron.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:01

Problem 96

Calculate the number of grams of mercury that contain the same number of atoms as $5.00 \mathrm{g}$ of tellurium.

Temi Ajayi
Temi Ajayi
Numerade Educator
04:35

Problem 97

Calculate the number of grams of lithium that contain the same number of atoms as $1.00 \mathrm{kg}$ of zirconium.

Temi Ajayi
Temi Ajayi
Numerade Educator
06:45

Problem 98

Given that the molar mass of carbon tetrachloride, $\mathrm{CCl}_{4},$ is $153.8 \mathrm{g},$ calculate the mass in grams of 1 molecule of $\mathrm{CCl}_{4}$.

Temi Ajayi
Temi Ajayi
Numerade Educator
10:26

Problem 99

Calculate the mass in grams of hydrogen present in 2.500 g of each of the following compounds.
a. benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$
b. calcium hydride, $\mathrm{CaH}_{2}$
c. ethyl alcohol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
d. serine, $\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{O}_{3} \mathrm{N}$

Temi Ajayi
Temi Ajayi
Numerade Educator
07:24

Problem 100

Calculate the mass in grams of nitrogen present in $5.000 \mathrm{g}$ of each of the following compounds.
a. glycine, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{O}_{2} \mathrm{N}$
b. magnesium nitride, $\mathrm{Mg}_{3} \mathrm{N}_{2}$
c. calcium nitrate
d. dinitrogen tetroxide

Temi Ajayi
Temi Ajayi
Numerade Educator
03:48

Problem 101

A strikingly beautiful copper compound with the common name "blue vitriol" has the following elemental composition: $25.45 \% \quad \mathrm{Cu}, \quad 12.84 \% \mathrm{S}$ $4.036 \% \mathrm{H}, 57.67 \%$ O. Determine the empirical formula of the compound.

Vasu Makani
Vasu Makani
Numerade Educator
03:54

Problem 102

A magnesium salt has the following elemental composition: $16.39\% $ Mg, $18.89\%$ N, $64.72\%$ O. Determine the empirical formula of the salt.

Temi Ajayi
Temi Ajayi
Numerade Educator
02:09

Problem 103

The mass $1.66 \times 10^{-24} \mathrm{g}$ is equivalent to 1 ___________.

Temi Ajayi
Temi Ajayi
Numerade Educator
04:37

Problem 104

Although exact isotopic masses are known with great precision for most elements, we use the average mass of an element's atoms in most chemical calculations. Explain.

Temi Ajayi
Temi Ajayi
Numerade Educator
06:15

Problem 105

Using the average atomic masses given in Table 8.1 calculate the number of atoms present in each of the following samples.
a. 160,000 amu of oxygen
b. 8139.81 amu of nitrogen
c. 13,490 amu of aluminum
d. 5040 amu of hydrogen
e. 367,495.15 amu of sodium

Temi Ajayi
Temi Ajayi
Numerade Educator
03:50

Problem 106

If an average sodium atom weighs 22.99 amu, how many sodium atoms are contained in $1.98 \times 10^{13}$ amu of sodium? What will $3.01 \times 10^{23}$ sodium atoms weigh?

Temi Ajayi
Temi Ajayi
Numerade Educator
11:07

Problem 107

Using the average atomic masses given inside the front cover of this text, calculate how many moles of each element the following masses represent.
a. $1.5 \mathrm{mg}$ of chromium
b. $2.0 \times 10^{-3} \mathrm{g}$ of strontium
c. $4.84 \times 10^{4}$ g of boron
d. $3.6 \times 10^{-6} \mu g$ of californium
e. 1.0 ton $(2000$ lb) of iron
f. $20.4 \mathrm{g}$ of barium
g. $62.8 \mathrm{g}$ of cobalt

Temi Ajayi
Temi Ajayi
Numerade Educator
06:06

Problem 108

Using the average atomic masses given inside the front cover of this text, calculate the mass in grams of each of the following samples.
a. 5.0 mol of potassium
b. 0.000305 mol of mercury
c. $2.31 \times 10^{-5}$ mol of manganese
d. 10.5 mol of phosphorus
e. $4.9 \times 10^{4}$ mol of iron
f. 125 mol of lithium
g. 0.01205 mol of fluorine

David Collins
David Collins
Numerade Educator
15:09

Problem 109

Using the average atomic masses given inside the front cover of this text, calculate the number of atoms present in each of the following samples.
a. $2.89 \mathrm{g}$ of gold
b. 0.000259 mol of platinum
c. 0.000259 g of platinum
d. 2.0 lb of magnesium
e. $1.90 \mathrm{mL}$ of liquid mercury (density $=13.6 \mathrm{g} / \mathrm{mL}$ )
f. 4.30 mol of tungsten
g. $4.30 \mathrm{g}$ of tungsten

Temi Ajayi
Temi Ajayi
Numerade Educator
13:02

Problem 110

Calculate the molar mass for each of the following substances.
a. ferrous sulfate
b. mercuric iodide
c. stannic oxide
d. cobaltous chloride
e. cupric nitrate

Temi Ajayi
Temi Ajayi
Numerade Educator
07:31

Problem 111

Calculate the molar mass for each of the following substances.
a. adipic acid, $\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O}_{4}$
b. caffeine, $\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}$
c. eicosane, $\mathrm{C}_{20} \mathrm{H}_{42}$
d. cyclohexanol, $\mathrm{C}_{6} \mathrm{H}_{11} \mathrm{OH}$
e. vinyl acetate, $\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}$
f. dextrose, $C_{6} \mathrm{H}_{12} \mathrm{O}_{6}$

Temi Ajayi
Temi Ajayi
Numerade Educator
06:31

Problem 112

Calculate the number of moles of the indicated substance present in each of the following samples.
a. $21.2 \mathrm{g}$ of ammonium sulfide
b. $44.3 \mathrm{g}$ of calcium nitrate
c. $4.35 \mathrm{g}$ of dichlorine monoxide
d. 1.0 Ib of ferric chloride
e. $1.0 \mathrm{kg}$ of ferric chloride

Temi Ajayi
Temi Ajayi
Numerade Educator
07:39

Problem 113

Calculate the number of moles of the indicated substance present in each of the following samples.
a. $1.28 \mathrm{g}$ of iron(II) sulfate
b. $5.14 \mathrm{mg}$ of mercury(II) iodide
c. $9.21 \mu g$ of tin(IV) oxide
d. 1.26 lb of cobalt(II) chloride
e. $4.25 \mathrm{g}$ of copper(II) nitrate

Temi Ajayi
Temi Ajayi
Numerade Educator
07:15

Problem 114

Calculate the mass in grams of each of the following samples.
a. $2.6 \times 10^{-2}$ mol of copper(II) sulfate, $\mathrm{CuSO}_{4}$
b. $3.05 \times 10^{3}$ mol of tetrafluoroethylene, $\mathrm{C}_{2} \mathrm{F}_{4}$
c. 7.83 mmol $(1 \mathrm{mmol}=0.001 \mathrm{mol})$ of 1,4 pentadiene, $\mathrm{C}_{5} \mathrm{H}_{8}$.
d. 6.30 mol of bismuth trichloride, $\mathrm{BiCl}_{3}$
e. 12.2 mol of sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$

Temi Ajayi
Temi Ajayi
Numerade Educator
05:30

Problem 115

Calculate the mass in grams of each of the following samples.
a. 3.09 mol of ammonium carbonate
b. $4.01 \times 10^{-6}$ mol of sodium hydrogen carbonate
c. 88.02 mol of carbon dioxide
d. 1.29 mmol of silver nitrate
e. 0.0024 mol of chromium(III) chloride

Temi Ajayi
Temi Ajayi
Numerade Educator
07:29

Problem 116

Calculate the number of molecules present in each of the following samples.
a. $3.45 \mathrm{g}$ of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
b. 3.45 mol of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
c. $25.0 \mathrm{g}$ of $\mathrm{ICl}_{5}$
d. $1.00 \mathrm{g}$ of $\mathrm{B}_{2} \mathrm{H}_{6}$
e. $1.05 \mathrm{mmol}$ of $\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}$

Temi Ajayi
Temi Ajayi
Numerade Educator
07:57

Problem 117

Calculate the number of moles of hydrogen atoms present in each of the following samples.
a. $2.71 \mathrm{g}$ of ammonia
b. 0.824 mol of water
c. $6.25 \mathrm{mg}$ of sulfuric acid
d. $451 \mathrm{g}$ of ammonium carbonate

Temi Ajayi
Temi Ajayi
Numerade Educator
18:23

Problem 118

Calculate the percent by mass of each element in the following compounds.
a. calcium phosphate
b. cadmium sulfate
c. iron(III) sulfate
d. manganese(II) chloride
e. ammonium carbonate
f. sodium hydrogen carbonate
g. carbon dioxide
h. silver(I) nitrate

Temi Ajayi
Temi Ajayi
Numerade Educator
07:17

Problem 119

Calculate the percent by mass of the element mentioned first in the formulas for each of the following compounds.
a. sodium azide, $\mathrm{NaN}_{3}$
b. copper(II) sulfate, $\mathrm{CuSO}_{4}$
c. gold(III) chloride, $\mathrm{AuCl}_{3}$
d. silver nitrate, $\mathrm{AgNO}_{3}$
e. rubidium sulfate, $\mathrm{Rb}_{2} \mathrm{SO}_{4}$
f. sodium chlorate, $\mathrm{NaClO}_{3}$
g. nitrogen triiodide, $\mathrm{NI}_{3}$
h. cesium bromide, $\operatorname{CsBr}$

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
13:56

Problem 120

Calculate the percent by mass of the element mentioned first in the formulas for each of the following compounds.
a. iron(II) sulfate
b. silver(I) oxide
c. strontium chloride
d. vinyl acetate, $\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}$
e. methanol, $\mathrm{CH}_{3} \mathrm{OH}$
f. aluminum oxide
g. potassium chlorite
h. potassium chloride

Temi Ajayi
Temi Ajayi
Numerade Educator
05:50

Problem 121

A $1.2569-g$ sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.7238 g; hydrogen, 0.07088 g: nitrogen, 0.1407 g: oxygen, 0.3214 g. Calculate the empirical formula of the compound.

Temi Ajayi
Temi Ajayi
Numerade Educator
02:35

Problem 122

A $0.7221-g$ sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.2990 g; hydrogen, 0.05849 g; nitrogen, 0.2318 g; oxygen, 0.1328 g. Calculate the empirical formula of the compound.

Abdel Osman
Abdel Osman
Numerade Educator
05:11

Problem 123

When $2.004 \mathrm{g}$ of calcium is heated in pure nitrogen gas, the sample gains $0.4670 \mathrm{g}$ of nitrogen. Calculate the empirical formula of the calcium nitride formed.

Temi Ajayi
Temi Ajayi
Numerade Educator
05:30

Problem 124

When $4.01 \mathrm{g}$ of mercury is strongly heated in air, the resulting oxide weighs $4.33 \mathrm{g}$. Calculate the empirical formula of the oxide.

Vishal Sharma
Vishal Sharma
Numerade Educator
04:15

Problem 125

When $1.00 \mathrm{g}$ of metallic chromium is heated with elemental chlorine gas, $3.045 \mathrm{g}$ of a chromium chloride salt results. Calculate the empirical formula of the compound.

Temi Ajayi
Temi Ajayi
Numerade Educator
04:36

Problem 126

When barium metal is heated in chlorine gas, a binary compound forms that consists of $65.95 \%$ Ba and $34.05 \%$ Cl by mass. Calculate the empirical formula of the compound.

Temi Ajayi
Temi Ajayi
Numerade Educator