Chemistry Chapter 3
CoCl2 * 6H2O
cobalt (II) chloride hexahydrate
CO(NO3)2 * 2H2O
cobalt (II) nitrate dihydrate
Co2(SO4)3
cobalt (III) sulfate
HIO3 (aq)
iodic acid
NiBr2 * 3H20
nickel (II) bromide trihydrate
NiCO3
nickel (II) carbonate
NiSO4 * 7H2O
nickel (II) sulfate heptahydrate
HNO3
nitric acid
NO2
nitrogen dioxide
NH3
nitrogen trihydride
NI3
nitrogen triiodide
OF2
oxygen difluoride
PCl5
phosphorus pentachloride
KHSO3
potassium hydrogen sulfite
Co(NO3)2
Cobalt (II) Nitrate
CuCO3
Copper (II) Carbonate
CuF2
Copper (II) fluoride
Li2CO3
Lithium Carbonate
CrBr2
Chromium (II) Bromide
(NH4)3PO4
ammonium phosphate
(NH4)2SO4
ammonium sulfate
Cr2S3
chromium (III) sulfide
N2O5
dinitrogen pentoxide
Na2CO3 * 10H20
sodium carbonate decahydrate
NaNO2
sodium nitrite
Na2SO4 * 7H2O
sodium sulfate heptahydrate
Copper
A certain metal hydroxide, M(OH)2, contains 32.8% oxygen by mass. What is the identity of the metal M?
6.66 mol of Carbon, 19.8 Hydrogen mol
A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound. How many moles of each element are in this sample?
80.0% Carbon, 20.0% Hydrogen
A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound. How many grams of each element are in this sample?
1.51×1023 molecules
A flask contains 0.250 mol of liquid bromine, Br2. Determine the number of bromine molecules present in the flask.
The molecular weight of C9H20 is 9*12 + 20*1 = 128 (grams/mole) and the carbon is 108/128 of that = 84.375% carbon and 15.625% hydrogen (84.28% Carbon , 15.72% Hydrogen) = 100%
A hydrocarbon is a compound that contains mostly carbon and hydrogen. Calculate the percent composition (by mass) of the following hydrocarbon: C9H20
AlCl3
Aluminum Chloride
NH4I
Ammonium Iodide
C4H6Ba04
Barium Acetate
Ionic usually have high melting points: 1)The solid in Bottle A: melts at 801 ∘C 3)The solid in bottle C melts at 825 ∘C Molecular usually have low melting points: 2)The solid in bottle B melts at 150 ∘C.
Based on the melting points, classify each compound as ionic or molecular. 1)The solid in Bottle A: melts at 801 ∘C 2)The solid in bottle B melts at 150 ∘C. 3)The solid in bottle C melts at 825 ∘C
CH3
Based on the mole ratio you determined in Part C, what is the empirical formula of this compound?
CaO3P
Calcium Phosphite
1.00 x10^24/6.02x10^23 = 1.661 moles 1 mol of H2O weighs 18g 1.661 * 18 = 29.9 g
Calculate the mass of 1.00×1024 (a septillion) molecules of water.
BeO
Enter the formula for the compound beryllium oxide.
Co3(PO4)2
Enter the formula for the compound cobalt(II) phosphate
5.563g CO2 * 1 molCO2 / 44.01g CO2 to get the amt of moles in CO2 .1264 mol CO2 * 1 mol C / 1 mol CO2 gets amt of C moles in 1 CO2 mol .1264 mol C 1.627 g H20 1.627 g H20 * 1 mol H20 / 18.016 g H2O gets amt of moles in H2O .0903 mol H2O* 2 mol H/1 mol H2O gets amt of H moles in 1 H20 mol .1806 mol H Now in order to find the oxygen you have to .1264 mol C * 12.01 g C/ 1 mol C = 1.518 g C .1806 mol H * 1.008 g H/ 1 mol H = .1820 g H Now subtract these values from the sample 1.893g - (1.518 g C + .1820 g H) = .193 Then Mol O = .193 g O * 1 mol O/ 16.00 g O = .0121 mol O Now divide all of the moles of C,H, and O by lowest value .1264 mol C/ .0121 mol O = 10.45 = 10.5 .1806 mol H/ .0121 mol O = 14.96 = 15 .0121 mol O/ .0121 mol O = 1= 1 so now you must get whole numbers so, you need 10.5 to be whole so, 10.5 *2 =21, now multiply everything by 2 the answer is C21H30O2
Find the molecular formula for progesterone.
Iron (III) Sulfate
Give the systematic name for the compound Fe2(SO4)3.
Magnesium Nitrate
Give the systematic name for the compound Mg(NO3)2
FePO4
Iron (III) Phosphate
Pb(CIO2)2
Lead (II) Chlorite
MgSO4
Magnesium Sulfate
magnesium sulfate heptahydrate
Name the hydrate MgSO4⋅7H2O.
Ni(BrO4)2
Nickel (II) Perbromate
NaBr
Sodium Bromide
Na2SO4
Sodium Sulfate
NaIO3
Sodium iodate
Sr(OH)2
Strontium Hydroxide
4.00g C4H10 x (1 mol C4H10)/(58.12g C4H10) = 0.068823 mol C4H10 second: convert moles to molecules(using avogadros number) 0.068823 mol C4H10 x (6.022x10^23 molecules C4H10)/(1 mol C4H10) = 4.14452x10^22 molecules C4H10 third: there are 4 carbon atoms in 1 molecule of butane, so use the following ratio: 4.14452x10^22 molecules C4H10 x (4 atoms C)/(1 molecule C4H10) = 1.66x10^23 atoms C (3 significant figures)
The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 4.00 g of butane?
P2O3
What is the empirical formula for the compound P4O6?
HClO2
What is the formula for chlorous acid?
H2SO3
What is the formula for sulfurous acid?
diboron hexahydride
What is the name for the compound B2H6?
phosphorus pentachloride
What is the name for the compound PCl5?
carbonic acid
What is the name of the acid whose formula is H2CO3?
Hydroiodic Acid
What is the name of the acid whose formula is HI?
ZnCl2
Zinc Chloride
BaBr2
barium bromide
BaCl2 * 2H2O
barium chloride dihydrate
Ba(OH)2 * H2O
barium hydroxide octahydrate
HBrO3 (aq)
bromic acid
CS2
carbon disulfide
H2CO3
carbonic acid
HCIO3
chloric acid
HClO2
chlorous acid
CuSO4 * 5H2O
copper (II) sulfate pentahydrate
B2Cl2
diboron dichloride
HCN (aq)
hydrocyanic acid
HF (aq)
hydrofluoric acid
HCI
hydrogen chloride
HF
hydrogen fluoride
HI (aq)
hydroiodic acid
HBrO (aq)
hypobromous acid
HCIO
hypochlorous acid
Fe(NO3)3 * 6H2O
iron (II) nitrate hexahydrate
FeSO3
iron (II) sulfite
FeCl3 * 2H2O
iron (III) chloride dihydrate
Fe2O3
iron (III) oxide
MgSO4 * 7H20
magnesium sulfate heptahydrate
Hg2SO4
mercury(I) sulfate
SiC
silicon carbide
SiO2
silicon dioxide
SiF4
silicon tetrafluoride
AgCn
silver cyanide
SF6
sulfur hexafluoride
SO3
sulfur trioxide
H2SO4 (aq)
sulfuric acid
H2SO3
sulfurous acid
P4O10
tetraphosphorus decoxide
P4S3
tetraphosphorus trisulfide
TiO2
titanium (IV) oxide
