Chapter 5. Chemical Composition
1. How many gidgets are present in 4.23 mol of gidgets?
2. How many mol are represented by 5.2 x 1072atoms of Fe?
3. a) What is the mass (in grams) of 9.01 mol of Ca?
b) How many mol are present in 21.2 g of Zn?
4. a) How many mol are present in 10.421 g of Fe?
b) What is the mass (in kilograms) of 905.25 mol of lead?
5. a) How many atoms are present in a 25.0 g sample of Na?
b) What is the mass (in grams) of 5.00 x 1025atoms of Cr?
6. How many atoms are present in 21.2 mg of Ag?
7. How many atoms are in a piece of gold measuring 1 cm x 2 cm x 0.5 cm?
(Density of gold is 19.32 g/mL)
8. The density of mercury (Hg) is 13.53 g/mL. How many litres will 4.2 x 1021atoms of Hg occupy?
9. What is the molar mass of Cu(SO4)2?
10. What is the molar mass of: a) H2O b) Ca3(PO4)2 c) C2H5OH
11. How many mol of O are present in 4.32 x 1032 molecules of Cu(SO4)2?
12. How many atoms of H are present in 4.2 mol of H2O?
13. How many grams of S are present in 32.1 grams of Cu(SO4)2?
14. How many grams of Ni are present in 50.0 g of NiNO3?
15. Complete the following conversions:
9.024 x 1023 Hg atoms = ____ g Hg
96.35 g NO = ____ molecules NO
253.52 g CO2= ____ TOTAL atoms
521.2 g (NH4)2Cr2O7 = _____ g H
1.371 g C2H5OH = ____ atoms of H
16. The hemoglobin content of blood is about 15.5 g/100 mL of blood. The molar mass of hemoglobin is about 64,500 g/mol and there are 4 iron atoms in a hemoglobin molecule. Approximately how many Fe atoms are present in 6 L of blood in a typical adult?
17. List the conversion factors, or combination of conversion factors that you would use in the following problem situations (no calculations required):
a) You need to go from g H2O to mol H2O
b) You need to go from mol H2SO4 to molecules H2SO4
c) From g HCl to molecules HCl
d) From mol KMnO4 to atoms O
e) From g KCN to g C
f) From mL CH3OH to mol CH3OH
g) From molecules NaCl to atoms Cl
h) From kg KBr to number of Br-ions
i) From mol H2SO4 to mL of H2SO4
j) From mol MgO to g O
k) From mm3 NaOH to mol NaOH
l) From molecules HCl to g H
m) From mol C in C6H6 to g C6H6
18. For all the situations in #17, calculate the final answer based on a starting unit of 5.
E.g.: for (a) How many mol H2O are in 5 g of H2O?
for (b) How many molecules of H2SO4 are in 5 mol H2SO4? etc…
NOTE: for f, i and k, the following densities are needed:
CH3OH d = 0.791 g/mL H2SO4 d = 1.45 g/mL NaOH d = 1.22 g/mL
19. Calculate the following:
a) Total number of ions in 38.1 g of CaF2 (hint… how many ions TOTAL are in one molecule of CaF2?)
b) Mass in g of 2.04 x 1021 molecules of N2O5
c) Mass in mg of 3.58 mol CuCl2
d) Mass in g of 9.64 x 1024 molecules of Cl2O7
20. Oxygen is required for metabolic combustion of foods. Calculate the number of atoms in 38.0 g of oxygen gas, the amount absorbed from the lungs at rest in about 15 minutes.
21. An imperial quart of oil is spilled on a lake. If the molecules were to spread out in an film one molecule deep, what would be the area of the oil slick, in square miles? The density of oil = 0.8g/mL ; area covered by one molecule = 0.5 nm2. Although oil is really a mixture of compounds of C & H, assume the oil is simply C16H34 and 1 qt = 1.1L and 1 mile = 1.6 km.
22. Why would it be necessary to clarify what you mean when you say “1 mole of nitrogen” or “1 mole of hydrogen”? Why is this clarification not necessary when referring to “1 mole of lead” or “1 mole of water”?
23. How many magnesium ions and how many nitride ions are in 4.75 mol of Mg3N2?
24. What mass of O2 contains the same number of moles of molecules as 52.0 g of N2?
25. What mass of sodium hydroxide (NaOH) contains the same number of moles as 126 g of nitric acid (HNO3)?
26. Ringer’s lactate is an aqueous (in water) physiological solution used for intraveneous fluid therapy. A 1.00 L sample of the solution contains 5.96 g of NaCl, 3.1 g of NaC3H5O3(sodium lactate), 0.3 g of KCl and 0.2 g CaCl2.
a) How many moles of each compound are in 1.00 L of solution?
b) The ingredients dissolve to form Na+, K+, Ca2+, Cl– and C3H5O3– ions. How many moles of each ion are in 1.00 L of solution. Note: there are several sources of Na+and Cl–.
27. The density of liquid benzene, C6H6 is 0.879 g/mL at 15oC. What is the volume in milliliters of 1.00 mol of benzene at this temperature?
28. A sample of 0.370 mol of a metal oxide (M2O3) weighs 55.4 g.
a) How many moles of O are in the sample?
b) How many grams of M are in the sample?
c) What element is represented by M?
29. a) How many grams of H2S are there in 0.400 moles of H2S?
b) How many grams of hydrogen and sulfur are contained in 0.400 moles of H2S?
c) How many molecules of H2S are contained in 0.400 moles of H2S?
d) How many atoms of H and S are contained in 0.400 moles of H2S?
30. a) How many moles of SO2 are represented by 9.54 g of SO2?
b) How many atoms of oxygen does this represent?
31. What is the average mass (in grams) of one oxygen atom?
32. What is the mass in grams of one molecule of CH3OH?
33. The density of gold is approx. 2 x 101 g/cm3. What is the volume of one gold atom?
34. How many moles are there in one atom?
35. What is the mass percent of each atom in (NH4)2Cr2O7?
36. Calculate the following mass percents:
a) Mass % of H in NH4HCO3 b) Mass % of Mn in KMnO4
37. Calculate the following mass fractions:
a) Mass fraction of Cl in CaCl2 b) Mass fraction of P in P4O7
38. The effectiveness of nitrogen fertilizer is determined mainly by its mass % N. Rank the following in terms of their effectiveness: KNO3; NH4NO3; Co(NH2)2; NH4SO4. Show your calculations.
39. A compound of iodine and cesium contains 63.94 g of metal and 61.06 g of nonmetal. How many grams of cesium are in 38.77 g of the compound? How many grams of iodine?
40. What is the empirical formula and the empirical formula molar mass of each of the following: a) C2H4 b) C2H6O2 c) N2O5 d) Ba3(PO4)2 e) Te4I16
41. What is the molecular formula of each of the following:
a) Empirical formula = CH2; molecular molar mass = 42.08 g/mol
b) EF = NH2; MMM = 32.05 g/mol
c) EF = NO2; MMM = 92.02 g/mol
d) EF = CHN; MMM = 135.14 g/mol
e) EF = CH; MMM = 78.11 g/mol
f) EF = C3H6O2; MMM = 74.08 g/mol
g) EF = C7H4O2; MMM = 240.02 g/mol
42. A 3.450 g sample of nitrogen reacts with 1.970 g of oxygen to form a compound. Determine the empirical formula for this compound.
43. A compound containing carbon, hydrogen and oxygen is found to be 40.00% carbon and 6.700% hydrogen by mass. The molar mass of the compound is between 115 g/mol and 125 g/mol. Determine the empirical formula and molecular formula of this compound.
44. Determine the empirical formula for the following situations:
a) 0.0630 mol of chlorine atom combined with 0.220 mol of oxygen atoms
b) 2.45 g silicon combined with 12.4 g of chlorine
c) a compound with 27.3% carbon and 72.7% oxygen by mass
d) a hydrocarbon (containing only C and H) which has 79.9% by mass C
45. A compound containing only silicon and chlorine contains 79.1% chlorine by mass and has a molar mass of 269 g/mol. What is the molecular formula?
46. A sample of 0.600 mole of metal reacts completely with fluorine to form 46.8 g of MF2.
a) How moles of F are in the sample of MF2 that formed?
b) How many grams of M are in this sample of MF2?
c) What element is represented by M?
47. A sample of nicotine contains 6.16 mmol of C, 8.56 mmol of H and 1.23 mmol of N. What is its empirical formula? (note: 1000 mmol = 1 mol)
48. Cortisol (molar mass = 362.47 g/mol), one of the major steroid hormones, is a key factor in the synthesis of protein. Its profound effect on the reduction of inflammation explains its use in the treatment of rheumatoid arthritis. Cortisol is 69.6% C, 8.34% H and 22.1% O by mass. What is its molecular formula?
49. 3.00g of molybdenum (Mo) combines with sulfur to produce 5.50 g of a compound. What is the empirical formula of this compound?
50. A 5.70 g sample of an iron oxide compound was heated in a stream of hydrogen gas, which reacted with the oxygen in the compound to form water. The water vapor was carried away in the stream of gas, leaving only pure metallic iron weighing 4.20g. Calculate the simplest possible formula for the original iron oxide.
51. When 2.31g of a carboxylic acid compound is burned in O2, the only products are 1.33g of H2O and 3.38g of CO2. Calculate the empirical (simplest possible) formula for this compound.
52. A compound was analyzed and found to have the following percentage composition: aluminum = 15.7%, sulfur = 28.11%, oxygen = 56.12%. The molar mass of the compound is known to be approximately 684 g/mol. What is the molecular formula?
1. 2.55 x 1024 gidgets
2. 8.6 x 1048 mol of Fe
3. a) 361 g of Ca b) 0.324 mol of Zn
4. a) 0.18660 mol of Fe b) 187.57 kg of Pb
5. a) 6.55 x 1023 atoms of Na b) 4.32 x 103 g of Cr
6. 1.18 x 1020 atoms
7. 6 x 1022 Au atoms
8. 1.0 x 10-4 L
9. 255.673 g/mol of Cu(SO4)2
10. a) 18.0152 g/mol b) 310.177 g/mol c) 46.069 g/mol
11. 5.74 x 109 mol of O
12. 5.1 x 1024 atoms of H
13. 8.05 g of S
14. 24.3 g of Ni
15. a) 300.6 g Hg
b) 1.934 x 1024 molecules of NO
c) 1.0407 x 1025 atoms
d) 16.67 g H
e) 1.075 x 1023 atoms
16. 3 x 1022 iron atoms
17. a) g H2O [latex]\longrightarrow[/latex] mol H2O using molar mass of H2O
b) mol H2SO4 [latex]\longrightarrow[/latex] molecules H2SO4 using Avogadro’s number
c) g HCl [latex]\longrightarrow[/latex] mol HCl using molar mass HCl [latex]\longrightarrow[/latex] molecules HCl using Avogadro’s number
d) mol KMnO4 [latex]\longrightarrow[/latex] mol O using chemical formula [latex]\longrightarrow[/latex] atoms O using Avogadro’s number
e) g KCN [latex]\longrightarrow[/latex] mol KCN using molar mass of KCN [latex]\longrightarrow[/latex] mol C using chemical formula [latex]\longrightarrow[/latex] g C using molar mass of C
f) mL CH3OH [latex]\longrightarrow[/latex] g CH3OH using density [latex]\longrightarrow[/latex] mol CH3OH using molar mass of CH3OH
g) molecules NaCl [latex]\longrightarrow[/latex] atoms Cl using formula ratio
molecules NaCl [latex]\longrightarrow[/latex] moles NaCl using Avogadro’s number [latex]\longrightarrow[/latex] moles Cl using the chemical formula [latex]\longrightarrow[/latex] atoms Cl using Avogadro’s number
h) kg KBr [latex]\longrightarrow[/latex] g KBr using metric conversions [latex]\longrightarrow[/latex] mol KBr using the molar mass of KBr [latex]\longrightarrow[/latex] moles Br– ions using chemical formula [latex]\longrightarrow[/latex] number of Br– ions using Avogadro’s number
i) mol H2SO4 [latex]\longrightarrow[/latex] g H2SO4 using molar mass of H2SO4 [latex]\longrightarrow[/latex] mL H2SO4 using density of H2SO4
j) mol MgO [latex]\longrightarrow[/latex] mol O using the chemical formula [latex]\longrightarrow[/latex] g O using molar mass of O
k) mm3 NaOH [latex]\longrightarrow[/latex] cm3 NaOH using metric conversions [latex]\longrightarrow[/latex] g NaOH using the density [latex]\longrightarrow[/latex] mol NaOH using the molar mass of NaOH
l) molecules HCl [latex]\longrightarrow[/latex] moles HCl using Avogadro’s number [latex]\longrightarrow[/latex] moles H using the chemical formula [latex]\longrightarrow[/latex] g H using the molar mass of H
m) mol C [latex]\longrightarrow[/latex] mol C6H6 using the chemical formula [latex]\longrightarrow[/latex] g C6H6 using the molar mass of C6H6
18. a) 0.3 mol b) 3 x 1024 molecules c) 8 x 1022 molecules
d) 1 x 1025 atoms e) 0.9 g f) 0.1 mol
g) 5 ions (or 5 atoms) h) 3 x 1025 ions i) 3 x 102 mL
j) 8 x 101 g k) 2 x 10-4 mol l) 8 x 10-24 g
m) 7 x 101 g
19. a) 8.82 x 1023 ions b) 0.366 g c) 4.81 x 105 mg
d) 2.93 x 103 g
20. 1.43 x 1024 atoms of O (7.15 x 1023 molecules O2)
21. 0.5 mile2
22. Because 1 mole of nitrogen may be 1 mole of N or 1 mole of N2, etc. Nitrogen and hydrogen (but not lead and water) are commonly found as diatomic molecules.
23 8.58 x 1024Mg2+ions and 5.72 x 1024N3-ions
24. 59.4 g of O2 (note: the nitrogen is given as N2)
25. 80.0 g of NaOH
26. a) 0.102 mol NaCl, 0.028 mol NaC3H5O3, 0.004mol KCl
and 0.002 mol CaCl2
b) Na+ = 0.130 mol, K+ = 0.004 mol, Ca2+ = 0.002,
Cl– = 0.110 mol; C3H5O3– = 0.028 mol
27. 88.9 mL
28. a) 1.11 mol O b) 37.6 g M c) V
29. a) 13.6 g H2S b) 0.806 g H, 12.8 g S
c) 2.41 x 1023 molecules H2S d) 4.82 x 1023H atoms and 2.41 x 1023 S atoms
30. a) 0.149 mol SO2 b) 1.79 x 1023atoms O
31. 2.65682 x 10-23 g
32. 5.3208 x 10-23 g
33. 2 x 10-23 cm3
34. 1.6605388 x 10-24 mol
35. N= 11.114%, H= 3.1990%, Cr= 41.256%, O= 44.431%
36. a) 6.3749% b) 34.7634%
37. a) 0.638883 b) 0.525222
38. NH4NO3> Co(NH2)2> KNO3 > NH4SO4
39. 19.83 g Cs, 18.94 g I
40. a) C2H4= CH2; 14.027 g/mol
b) C2H6O2= CH3O; 31.034 g/mol
c) N2O5= N2O5; 108.0104 g/mol
d) Ba3(PO4)2= Ba3(PO4)2; 601.924 g/mol
e) Te4I16= TeI4; 635.22 g/mol
41. a) C3H6 b) N2H4 c) N2O4
d) C5H5N5 e) C6H6 f) C3H6O2
43. EF = CH2O, MF = C4H8O4
44. a) Cl2O7 b) SiCl4 c) CO2 d) CH3
46. a) 1.20 mol F b) 24.0 g M c) Ca
50. Fe4O5(Fe8O10etc. are also possible, but not the simplest)
51. CH2O (Note that, based on the products, the unknown compound could only contain C, H and O, and note that all of the C in the original compound ends up in the CO2and all the H ends up in the H2O.)