Chemistry...
For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. MISSED THIS? Read Section 4.3; Watch KCV 4.3, IWE 4.4 a. Ba(s)_ + Cl2(g) → BaCl2(s) b. CaO(s)_ + CO2(g) → CaCO3(s) c. 2 Mg(s)_ + O2(g) → 2 MgO(s) d. 4 Al(s)_ + 3 O2(g) → 2 Al2O3(s)
5.56 g BaCl25.56 g BaCl2 6.55 g CaCO36.55 g CaCO3 6.09 g Mg O 6.93 g Al2O3
Two samples of the same compound containing elements A and B are decomposed. The first sample produces 15 g A and 35 g B. The second sample produces 25 g of A and what mass of B?
58gB
The U.S. Food and Drug Administration (FDA) recommends that an adult consume less than 2.4 g of sodium per day. What mass of sodium chloride (in grams) can you consume and still be within the FDA guidelines? Sodium chloride is 39% sodium by mass.
6.2g NaCl
What mass (in grams) of iron(III) oxide contains 58.7 g of iron? Iron(III) oxide is 69.94% iron by mass.
83.9 g Fe2O3
2 A(aq) + B(aq) → C(aq) What is the limiting reactant if we mix equal volumes of a 1 M solution of A and a 1 M solution of B?
A
For the reaction shown here, 3.5 mol A is mixed with 5.9 mol B and 2.2 mol C. What is the limiting reactant? 3 A + 2 B + C → 2 D
A
Which statement best explains the difference between a law and a theory?
A law summarizes a series of related observations; a theory gives the underlying reasons for them
Write the formula for the ionic compound that forms between aluminum and oxygen
Al2O3
Write the formula for the compound formed between aluminum and nitrogen.
AlN
10,000m How many sig figs?
Ambiguous; probably one, but dont know
Upon combustion, a 0.8233-g sample of a compound containing only carbon, hydrogen, and oxygen produces 2.445 g CO2 and 0.6003 g H2O. Find the empirical formula of the compound.
C10H12O
Write the balanced chemical equation for the fermentation of sucrose (C12H22O11) by yeasts in which the aqueous sugar reacts with water to form aqueous ethanol (C2H5OH) and carbon dioxide gas.
C12H22O11(s)+H2O(l)−→−4 C2H5OH(aq)+4 CO2(g)
Upon combustion, a compound containing only carbon and hydrogen produces 1.60 g CO2 and 0.819 g H2O. Find the empirical formula of the compound.
C2H5
Write complete ionic and net ionic equations for the reaction. 3 SrCl2(aq)+2 Li3PO4(aq) −→− Sr3(PO4)2(s)+6 LiCl(aq)
Complete ionic: 3Sr2+(aq) + 6Cl-(aq) + 6Li+(aq) + 2PO43-(aq) -> Sr3(PO4)2(s) + 6Li+(aq) + 6Cl-(aq) Net ionic: 3Sr+(aq) + 2PO4-(aq) -> Sr3(PO4)2(s)
TiO2(s)+2 C(s)→Ti(s)+2CO(g) When 28.6 kg of C reacts with 88.2 kg of TiO2, 42.8 kg of Ti is produced. Find the limiting reactant, theoretical yield (in kg), and percent yield.
Limiting Reactant: TiO2 Theoretical Yield: 52.9kg Percent yield: 80.9%
Name the compound Li2Cr2O7
Lithium Dichromate
Classify the substance as an atomic element, molecular element, molecular compound, or ionic compound: Bromine
Molecular Element (Br2)
How do you describe lead?
Pb, Metal, main group element
Write the balanced chemical equation for each reaction. MISSED THIS? Read Section 4.2; Watch KCV 4.2, IWE 4.2 a.Solid lead(II) sulfide reacts with aqueous hydrobromic acid to form solid lead(II) bromide and dihydrogen monosulfide gas. b.Gaseous carbon monoxide reacts with hydrogen gas to form gaseous methane (CH4CH4) and liquid water. c.Aqueous hydrochloric acid reacts with solid manganese(IV) oxide to form aqueous manganese(II) chloride, liquid water, and chlorine gas. d.Liquid pentane (C5H12C5H12) reacts with gaseous oxygen to form carbon dioxide and liquid water.
PbS(s)+2 HBr(aq)−→−PbBr2(s)+H2S(g) CO(g)+3 H2(g)−→−CH4(g)+H2O(l) 4 HCl(aq)+MnO2(g)−→−MnCl2(aq)+2 H2O(l)+Cl2(g) C5H12(l)+8 O2(g)−→−5 CO2(g)+6 H2O(g)
Write the formula for rubidium sulfide.
Rb2S
Write the formula for ruthenium(IV) oxide.
RuO2
Which metal has the same charge in all of its compounds? Fe, Mo, Pb, Sr
Sr
Write a balanced chemical equation for the reaction of solid strontium with iodine gas.
Sr(s)+I2(g)−→−SrI2(s)
What is the net ionic equation for the reaction that occurs when you mix aqueous solutions of KOH and SrCl2?
Sr2 + (aq) + 2 OH−(aq) → Sr(OH)2(s)
Which statement best captures one of the differences between the law of definite proportions and the law of multiple proportions?
The law of definite proportions applies to two or more samples of the same compound while the law of multiple proportions applies to two different compounds containing the same two elements (A and B)
What are the atomic number, mass number, and symbol for the carbon isotope with seven neutrons? How many protons and neutrons are present in an atom of K1939K1939?
Z=6,A=13,C613Z=6,A=13,C613 19 protons, 20 neutrons
a.sweat b.carbon dioxide c.aluminum d.vegetable soup
a.sweat b.carbon dioxide c.aluminum d.vegetable soup
0.00002 m How many sig figs?
1
Calculate the formula mass of calcium nitrate.
164.10 amu
How many sig figs? 0.04450
4
[(28.7×105)÷48.533]+144.99
5.93*10^4
4.562 * 3.99870 / (452.6744 - 452.33)
53
How many mols of a solute are required to make 3.0L of a 2M solution
6mols
(12.01 × 0.3) + 4.811
8
Name the compound CaBr2
Calcium bromide
Name N2O5
Dinitrogen pentaoxide
Which of the ions listed below is a spectator ion in the complete ionic equation shown here? Ag+(aq) + NO3- (aq) + Na+(aq) + I−(aq) → AgI (s) + NO3- (aq) + Na+(aq)
NO3- and Na(aq)
Name the compound: NI3
Nitrogen triiodide
Name HClO4(aq)
Perchloric acid
Which element contains 43 protons?
Tc
How many sig figs? 10dm = 1m
Unlimited sig figs
Name HC2H3O2(aq)
acetic acid
Name the compound FeS.
iron(II) sulfide
Predict whether each compound is soluble or insoluble. Ca(NO3)2
soluble
Name the compound Sn(ClO3)2.
tin(II) chlorate
Which change is a physical change? a. wood burning b. iron rusting c. dynamite exploding d. gasoline evaporating
d
Name the acid HF(aq).
hydrofluoric acid
Classify each compound as organic or inorganic. MISSED THIS? Read Section 3.11 a.CaCO3 b.C4H8 c.C4H6O6 d.LiF
inorganic organic organic inorganic
A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: MISSED THIS? Read Section 4.3, 5.3; Watch KCV 4.3, IWE 4.6, 5.4 2 KCl(aq)+Pb(NO3)2(aq) −→− PbCl2(s)+2 KNO3(aq)
lead nitrate, 3.75 g, 65.3%
Name the compound Pb(C2H3O2)2
lead(II) acetate
a.colorless b.flammable c.liquid at room temperature d.density = 0.79 g/mL e.mixes with water
physical, chemical, physical, physical, physical
Refer to the nomenclature flowchart (Figure 3.11) to name each compound. MISSED THIS? Read Section 3.7 ; Watch IWE 3.11 a.KClO3 b.I2O5 c.PbSO4
potassium chlorate diiodine pentoxide lead(II) sulfate
Name the compound Ag3N
silver nitride
Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. MISSED THIS? Read Section 5.4; Watch IWE 5.5 a.AgNO3 b.Pb(C2H3O2)2 c.KNO3 d.(NH4)2S
soluble Ag+,NO3− soluble Pb2+,C2H3O2− soluble K+,NO3− soluble NH4+,S2−
Refer to the nomenclature flowchart (Figure 3.11) to name each compound. MISSED THIS? Read Section 3.7 ; Watch IWE 3.11 a.SrCl2SrCl2 b.SnO2SnO2 c.P2S5P2S5 d.HC2H3HC2H3O2O2(aq)
strontium chloride tin(IV) oxide diphosphorus pentasulfide acetic acid
Name H2SO3(aq)
sulfurous acid
Name the compound: P4S10
tetraphosphorous decasulfide
To what volume should you dilute 0.200 L of a 15.0 M NaOH solution to obtain a 3.00 M NaOH solution?
0.2(15) = 3(v2) v2 = 1L
The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g of NH3.
0.333 g PH3
Calculate the amount of copper (in moles) in a 35.8 g pure copper sheet.
0.563 mol Cu
Perform calculation to correct num of sig figs: 1.10 x 0.5120 x 4.0015 / 3.4555
0.652
Solid potassium chlorate (KClO3) decomposes into potassium chloride and oxygen gas when heated. How many moles of oxygen form when 55.8 g of KClO3 completely decomposes?
0.683 mol O2
An aluminum sphere contains 8.55 x 10^22 Aluminum atoms. What is the sphere's radius in centimeters? Density of Al is 2.7 g/cm^3
0.697 cm
Find the radius (r) of an aluminum cylinder that is 2.00 cm long and has a mass of 12.4 g. For a cylinder, V=πr2l.
0.855 cm
Determine whether each reaction is an oxidation-reduction reaction. For each oxidation-reduction reaction, identify the oxidizing agent and the reducing agent. 2 Mg(s)+O2(g) −→− 2 MgO(s) 2 HBr(aq)+Ca(OH)2(aq) −→− 2 H2O(l)+CaBr2(aq) Zn(s)+Fe2+(aq) −→− Zn2+(aq)+Fe(s)
1. Yes, O2 is oxidizing agent, Mg is reducing agent 2. No 3. Yes, Fe2+ is oxidizing agent, Zn is reducing agent
Backpackers often use canisters of white gas to fuel a cooking stove's burner. If one canister contains 1.45 L of white gas and the density of the gas is 0.710 g/cm3, what is the mass of the fuel in kilograms?
1.03kg
How many molecules in 325 mg of C9H8O4
1.09 x 10^21
2.5110 × 21.20 ÷ (44.11 + 1.223)
1.174
How many electrons in O2-
10
Write a molecular equation for the gas-evolution reaction that occurs when you mix aqueous nitric acid and aqueous sodium carbonate.
2 HNO3(aq)+Na2CO3(aq) −→− H2O(l)+CO2(g)+2 NaNO3(aq)
Write a balanced chemical equation for the reaction of solid lithium with liquid water.
2 Li(s)+2 H2O(l)−→−2 Li+(aq)+2 OH−(aq)+H2(g)
In a popular classroom demonstration, solid sodium is added to liquid water and reacts to produce hydrogen gas and aqueous sodium hydroxide. Write the balanced chemical equation for this reaction.
2 Na(s)+2 H2O(l)−→−H2(g)+2 NaOH(aq)
An argon isotope has mass number 40. How many neutrons does it have?
22
Another component of acid rain is nitric acid, which forms when NO2, also a pollutant, reacts with oxygen and water according to the simplified equation: 4 NO2(g)+O2(g)+2 H2O(l)→4 HNO3(aq) The generation of the electricity used by a medium-sized home produces about 16 kg of NO2 per year. Assuming that there is adequate O2 and H2O, what mass of HNO3, in kg, can form from this amount of NO2 pollutant?
22 kg HNO3
If we dissolve 25 g of salt in 251 g of water, what is the mass of the resulting solution?
276g
Write a balanced equation for the combustion of gaseous butane (C4H10) a fuel used in portable stoves and grills, in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water.
2C4H10 + 13O2 -> 8CO2 + 10H2O
Begin by writing an unbalanced equation showing the reaction of CH3OH with O2 to form CO2 and H2O.
2CH3OH + 3O2 -> 2CO2 + 4H2O
Write a balanced equation for the reaction between solid cobalt(III) oxide and solid carbon to produce solid cobalt and carbon dioxide gas.
2Co2O3 + 3C -> 4Co + 3CO2
How many sig figs? 554 km
3
Laboratory calls for 3L of a 0.5M CaCl2 solution. How should we prepare this from a 10M stock solution?
3(0.5) = 10M(v2) v2 = 0.15L
Write a balanced equation for the reaction between aqueous strontium chloride and aqueous lithium phosphate to form solid strontium phosphate and aqueous lithium chloride.
3SrCl2(aq) + 2LiPo4(aq) -> Sr3(PO4)2(s) + 6LiCl(aq)
How many sig figs? 1.000 x 10^5
4
Find amount of CO2 molecules in 10.8grams
1.48 x 10^23 molecules
How many copper atoms are in a copper penny with a mass of 3.1 grams
2.94 x 10^22 atoms
Calculate the average mass, in grams, of one platinum atom.
3.239 x 10^-22 g
The empirical formula of butanedione is C2H3O, and its molar mass is 86.09 g/mol. Determine its molecular formula.
C4H6O2
What type of bond—ionic or covalent—forms between nitrogen and oxygen?
Covalent
P or C? A copper wire is hammered flat
P
P or C? Formation of frost
P
Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. MISSED THIS? Read Section 5.9 a.4 Li(s)+O2(g) −→− 2 Li2O(s) b.Mg(s)+Fe2+(aq) −→− Mg2+(aq)+Fe(s) c.Pb(NO3)2(aq)+Na2SO4(aq) −→− PbSO4(s)+2 NaNO3(aq) d.HBr(aq)+KOH(aq) −→− H2O(l)+KBr(aq)
redox reaction, oxidizing agent: O2 reducing agent: Li redox reaction, oxidizing agent: Fe2+ reducing agent: Mg not a redox reaction not a redox reaction
63.What is the oxidation state of Cr in each compound? MISSED THIS? Read Section 5.9; Watch IWE 5.13 a.CrO b.CrO3 c.Cr2O3
+2 +6 +3
What is the oxidation state of carbon in CO32−
+4
Assign an oxidation state to each atom in each element, ion, or compound. Cl2 Na+ KF CO2 SO42− K2O2
0 +1 +1/-1 (sum is 0) +4/-2(2) (sum is 0) +6/4(-2) (sum is -2) +1(2)/-1(2) (sum is 0)
(43.998 × 0.00558) ⁄ 2.002
0.121
What is the molarity of a solution containing 25.5 g KBr dissolved in enough water to make 1.75 L of solution?
0.122M
The titration of 15.00 mL of HBr solution of unknown concentration requires 18.44 mL of a 0.100 M KOH solution to reach the equivalence point. What is the concentration of the unknown HBr solution in M?
0.123M
The titration of 10.00 mL of HCl solution of unknown concentration requires 12.54 mL of a 0.100 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M?
0.125M HCl
Convert 1,285 cm2 to m2
0.1285 m^2
What is the molarity of NO3− in each solution? MISSED THIS? Read Sections 5.2, 5.4; Watch KCV 5.2, IWE 5.1 a.0.150 M KNO3 b.0.150 M Ca(NO3)2 c.0.150 M Al(NO3)3
0.150 M NO3− 0.300 M NO3− 0.450 M NO3−
(8.01 − 7.50) ⁄ 3.002
0.17
A 25.00-mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is MISSED THIS? Read Section 5.7; Watch IWE 5.11 HClO4(aq)+NaOH(aq) −→− H2O(l)+NaClO4(aq)
0.1810 M HClO4
What volume (in L) of a 0.150 M KCl solution will completely react with 0.150 L of a 0.175 M Pb(NO3)2 solution according to the following balanced chemical equation? 2 KCl(aq)+Pb(NO3)2(aq) −→− PbCl2(s)+2 KNO3(aq)
0.350L KCl
How many moles of KCl are contained in each solution? MISSED THIS? Read Section 5.2; Watch KCV 5.2, IWE 5.2 a.0.556 L of a 2.3 M KCl solution b.1.8 L of a 0.85 M KCl solution c.114 mL of a 1.85 M KCl solution
1.3 mol 1.5 mol 0.211 mol
Two samples of carbon monoxide are decomposed into their constituent elements. One sample produces 17.2 g of oxygen and 12.9 g of carbon, and the other sample produces 10.5 g of oxygen and 7.88 g of carbon. Show that these results are consistent with the law of definite proportions.
1.33:1
How many fluorine atoms are present in 5.85 g of C2F4?
1.41×1023 F atoms
Calculate the number of Copper atoms in 2.45 mol Copper
1.48 x 10^24 atoms
A 7.83 g sample of HCN contains 0.290 g of H and 4.06 g of N. Find the mass of carbon in a sample of HCN with a mass of 3.37 g.
1.50g
How many molecules of ethanol (C2H5OH) (the alcohol in alcoholic beverages) are present in 145 mL of ethanol? The density of ethanol is 0.789g/cm3.
1.50×10241.50×1024 molecules EtOH
Determine the number of CH2Cl2 molecules are there in 25.0 g of CH2Cl2
1.77 x 10^23 molecules
How many 1-cm squares would it take to construct a square that is 1 m on each side?
10,000
Potassium iodide reacts with lead(II) nitrate in this precipitation reaction: 2 KI(aq) + Pb(NO3)2(aq) → 2 KNO3(aq) + PbI2(s) What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all of the lead in 155.0 mL of a 0.112 M lead(II) nitrate solution?
174mL
Calculate the formula mass of Glucose (C6H12O6)
180.16 amu
Write a balanced chemical equation for each reaction. the reaction between aluminum metal and chlorine gas the reaction between lithium metal and liquid water the reaction between gaseous hydrogen and liquid bromine
2 Al(s)+3 Cl2(g)→2 AlCl3(s) 2 Li(s)+2 H2O(l)→2 Li+(aq)+2 OH−(aq)+H2(g) H2(g)+Br2(l)→2 HBr(g)
Write a balanced equation for the complete combustion of liquid C2H5SHC2H5SH. Hint: The sulfur in this compound reacts to form SO2SO2.
2 C2H5SH(l)+9 O2(g)→4 CO2(g)+2 SO2(g)+6 H2O(g)
Complete and balance each gas-evolution equation. MISSED THIS? Read Section 5.8; Watch KCV 5.5 a.HBr(aq)+NiS(s) −→− b.NH4I(aq)+NaOH(aq) −→− c.HBr(aq)+Na2S(aq) −→− d.HClO4(aq)+Li2CO3(aq) −→−
2 HBr(aq)+NiS(s)−→−H2S(g)+NiBr2(aq)2 NH4I(aq)+NaOH(aq)→H2O(l)+NH3(g)+NaI(aq) 2 HBr(aq)+Na2S(aq)−→−H2S(g)+2 NaBr(aq) 2 HClO4(aq)+Li2CO3(aq)−→−H2O(l)+CO2(g)+2 LiClO4(aq)
Sulfuric acid is a component of acid rain formed when gaseous sulfur dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous sulfuric acid. Write the balanced chemical equation for this reaction. (Note: This is a simplified representation of this reaction.)
2 SO2(g)+O2(g)+2 H2O(l)−→−2 H2SO4(aq)
How many liters of a 0.125 M NaOH solution contain 0.255 mol of NaOH?
2.04L solution
What is the minimum amount of 6.0 M H2SO4H2SO4 necessary to produce 25.0 g of H2(g)H2(g) according to the reaction between aluminum and sulfuric acid? MISSED THIS? Read Section 5.3; Watch IWE 5.4 2 Al(s)+3 H2SO4(aq) −→− Al2(SO4)3(aq)+3 H2(g)
2.1 L
Calculate the amount of Carbon (in mols) contained in 0.0265 g Carbon
2.21 x 10^-3 mol C
Find the density, in g/cm3, of a metal cube with a mass of 50.3 g and an edge length (l) of 2.65 cm. For a cube, V=l3
2.70g/cm^3
A drop of gasoline has a mass of 22 mg and a density of 0.754 g/cm3. What is its volume in cubic centimeters?
2.9 * 10^-2cm^3
Find the number of atoms in a copper rod with a length of 9.85 cm and a radius of 1.05 cm. The density of copper is 8.96 g/cm3
2.90×1024 Cu atoms
A 10.0 mL sample of 0.20 M HBr solution is titrated with 0.10 M NaOH. What volume of NaOH is required to reach the equivalence point?
20 mL
Sulfur and fluorine react to form sulfur hexafluoride. S(s) + 3 F2(g) → SF6(g) If 50.0 g S reacts as completely as possible with 105.0 g F2(g), what mass of the excess reactant remains?
20.5gS
Gallium has two naturally occurring isotopes: Ga-69 with a mass of 68.9256 amu and a natural abundance of 60.11%, and Ga-71. Use the atomic mass of gallium from the periodic table to find the mass of Ga-71.
24.31amu
6 CO2(g)+6 H2O(l)−→−−− 6 O2(g)+C6H12O6(aq) Suppose that a particular plant consumes 37.8 g of CO2 in one week. Assuming that there is more than enough water present to react with all of the CO2, what mass of glucose (in grams) can the plant synthesize from the CO2?
25.8grams C6H12O6
How many mols of O2 are required to react with 22 moles of C8H18 according to the balanced chemical equation for the combustion of octane?
275 mol O2
Gallium is a solid metal at room temperature, but it will melt to a liquid in your hand. The melting point of gallium is 85.6 °F. What is this temperature on (a) the Celsius scale and (b) the Kelvin scale?
29.8ºF, 302.9K
Write a balanced chemical equation for each reaction. the reaction between potassium metal and bromine gas the reaction between rubidium metal and liquid water the reaction between gaseous chlorine and solid iodine
2K(s)+Br2(g)->2KBr(s) 2Rb(s)+2H2O(l)->2Rb+(aq)+2OH-(aq)+H2(g) Cl2(g)+I2(s)->2ICl(g)
Suppose that one of Millikan's oil drops has a charge of -4.8 × 10-19 C. How many excess electrons does the drop contain?
3
A vineyard has 145 acres of Chardonnay grapes. A particular soil supplement requires 5.50 g for every square meter of vineyard. How many kilograms of the soil supplement are required for the entire vineyard? (1 km2=247 acres)
3.23 * 10^3kg
Express the quantity 33.2 × 10−4 m in mm
3.32mm
Butane (C4H10) is the liquid fuel in lighters. How many grams of carbon are present within a lighter containing 7.25 mL of butane? (The density of liquid butane is 0.601 g/mL.)
3.60 g C
A compound containing only carbon and hydrogen has a carbon-to-hydrogen mass ratio of 11.89. Which carbon-to-hydrogen mass ratio is possible for another compound composed only of carbon and hydrogen? 2.5 3.97 4.66 7.89
3.97
Consider the precipitation reaction: MISSED THIS? Read Section 5.3; Watch IWE 5.4 2 Na3PO4(aq)+3 CuCl2(aq) −→− Cu3(PO4)2(s)+6 NaCl(aq) What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2
37.1 mL
2 SO2(g)+O2(g)+2 H2O(l)→2 H2SO4(aq) The generation of the electricity used by a medium-sized home produces about 25 kg of SO2 per year. Assuming that there is more than enough O2 and H2O, what mass of H2SO4, in kg, can form from this much SO2?
38kg H2SO4
Mg(OH)2(s) + 2 HCl(aq) → 2 H2O(l) + MgCl2(aq) What mass of HCl, in grams, is neutralized by a dose of milk of magnesia containing 3.26 g Mg(OH)2?
4.08g HCl
. Determine the mass of oxygen in a 7.2-g sample of Al2(SO4)3.
4.0gO
What mass of hydrogen (in grams) is contained in 1.00 gallon of water? (The density of water is 1.00 g/mL.)
4.23 x 10^2gH
A pure silver ring contains 2.80×1022 silver atoms. How many moles of silver atoms does it contain?
4.65×10−2 mol Ag
An α particle, He2+4, has a mass of 4.00151 amu. Find the value of its charge-to-mass ratio in C/kg
4.82241 x 10^7C/kg
Perform calculation to correct num of sig figs: 0.355 + 105.1 - 100.5820
4.9
How many grams of sucrose (C12H22O11) are in 1.55 L of 0.758 M sucrose solution?
402g
2NO(g)+5 H2(g)→2 NH3(g)+2 H2O(g) Starting with 86.3 g NO and 25.6 g H2, find the theoretical yield of ammonia in grams.
49g NH3
How many sig figs? 5.0003
5
What volume (in mL) of a 0.150 M HNO3 solution will completely react with 35.7 mL of a 0.108 M Na2CO3 solution according to the following balanced chemical equation? Na2CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO2(g) + H2O(l)
51.4mL HNO3
What volume (in mL) of a 0.150 M HNO3 solution will completely react with 35.7 mL of a 0.108 M Na2CO3 solution according to the following balanced chemical equation? Na2CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO2(g) + H2O(l)
51.4mL HNO3 solution
Acetic acid (HC2H3O2) is the active ingredient in vinegar. Calculate the mass percent composition of oxygen in acetic acid.
53.29%
Calculate the mass of 2.25×10222.25×1022 tungsten atoms.
6.87 g W
Copper has two naturally occurring isotopes: Cu-63 with a mass of 62.9291 amu and a natural abundance of 69.17%, and Cu-65 with a mass of 64.9278 amu and a natural abundance of 30.83%. Calculate the atomic mass of copper.
63.55 amu
Calculate the mass percent of Cl in C2Cl4F2
69.58%
Calculate the mass percent composition of sodium in sodium oxide
74.19% Na
Hydrobromic acid dissolves solid iron according to the reaction: Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g) What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?
9.3 g HBr,0.12 g H2
Assign oxidation states to each atom in each element, ion, or compound. MISSED THIS? Read Section 5.9; Watch IWE 5.13 a.Ag b.Ag+ c.CaF2 d.H2S e.CO32− f.
Ag: 0 Ag: +1 Ca: +2, F: −1 H: +1, S: −2 C: +4, O: −2 Cr: +6, O: −2
Classify the substance as an atomic element, molecular element, molecular compound, or ionic compound: Xenon
Atomic Element
P or C? A match ignites when struck on flint
C
P or C? A nickel dissolves in acid to form a blue-green solution
C
P or C? Bleaching of hair with hydrogen peroxide
C
P or C? Burning of lamp oil
C
Upon combustion, a 0.8009-g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6004 g CO2 and 0.6551 g H2O. Find the empirical formula of the compound.
C2H4O
Determine the molecular formula for the compound with a molar mass of 60.10 g/mol and the following percent composition: C,39.97%H,13.41%N,46.62%
C2H8N2
The ratio of oxygen to carbon by mass in carbon monoxide is 1.33:1.00. Find the formula of an oxide of carbon in which the ratio by mass of oxygen to carbon is 2.00:1.00.
C2O3
Upon combustion, a compound containing only carbon and hydrogen produces 1.83 g CO2 and 0.901 g H2O. Find the empirical formula of the compound.
C5H12
A laboratory analysis of aspirin determines the following mass percent composition: C 60.00%; H 4.48%; O 35.52% Find the empirical formula.
C9H8O4
A sample of a compound is decomposed in the laboratory and produces 165 g carbon, 27.8 g hydrogen, and 220.2 g oxygen. Calculate the empirical formula of the compound.
CH2O
Write the formula based on the name, or the name based on the formula, for each hydrocarbon. MISSED THIS? Read Section 3.11 a.propane b.CH3CH2CH3CH3CH2CH3 c.octane d.CH3CH2CH2CH2CH3
CH3CH2CH3CH3CH2CH3 propane CH3CH2CH2CH2CH2CH2CH2CH3CH3CH2CH2CH2CH2CH2CH2CH3 pentane
Write a balanced equation for the combustion of liquid methyl alcohol (CH3OH).
CH3OH(l)+O2(g) -> CO2(g) + H2O(g) 2CH3OH(l)+3O2(g)->2CO2(g)+4H2O(g)
Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s)+3CO(g)→2Fe(s)+3 CO2(g)Fe2O3(s)+3CO(g)→2Fe(s)+3 CO2(g) The reaction of 167 g Fe2O3 with 85.8 g CO produces 72.3 g Fe. Determine the limiting reactant, theoretical yield, and percent yield.
CO is the limiting reagent, since it only produces 114 g Fe. Therefore, 114 g Fe is the theoretical yield: percentage yield=63.4% yield.
Write the formula for the ionic compound that forms between Calcium and oxygen
CaO
Write formula for Cobalt(III) oxide
Co2O3
Write the formula for cobalt(II) phosphate.
Co3(PO4)2
Name CoF2
Cobalt(II) fluoride
Write balanced complete ionic and net ionic equations for each acid-base reaction. MISSED THIS? Read Section 5.7; Watch KCV 5.5, IWE 5.9 a.HBr(aq)+NaOH(aq) −→− b.HF(aq)+NaOH(aq) −→− c.HC2H3O2(aq)+RbOH(aq) −→−
Complete ionic: H+(aq)+Br−(aq)+Na+(aq)+OH−(aq)−→−H2O(l)+Na+(aq)+Br−(aq) Net ionic: H+(aq) OH−(aq)−→−H2O(l) Complete ionic: HF(aq)+Na+(aq)+OH−(aq)−→−H2O(l)+Na+(aq)+F−(aq) Net ionic: HF(aq)+OH−(aq)−→−H2O(l)+F−(aq) Complete ionic: HC2H3O2(aq)+Rb+(aq)+OH−(aq)−→−H2O(l)+Rb+(aq)+C2H3O −2(aq) Net ionic: HC2H3O2(aq)+OH−(aq)−→−H2O(l)+C2H3O −2(aq)
Write balanced complete ionic and net ionic equations for each reaction. MISSED THIS? Read Section 5.6 a.HCl(aq)+LiOH(aq) −→− H2O(l)+LiCl(aq) b.CaS(aq)+CuCl2(aq) −→− CuS(s)+CaCl2(aq) c.NaOH(aq)+HC2H3O2(aq) −→− H2O(l)+NaC2H3O2(aq) d.Na3PO4(aq)+NiCl2(aq) −→− Ni3(PO4)2(s)+NaCl(aq)
Complete: H+(aq)+Cl−(aq)+Li+(aq)+OH−(aq)−→−H2O(l)+Li+(aq)+Cl−(aq) Net: H+(aq)+OH−(aq)−→−H2O(l) Complete: Ca2+(aq)+S2−(aq)+Cu2+(aq)+2Cl−(aq)−→−CuS (s)+Ca2+(aq)+2Cl−(aq) Net: Cu2+(aq)+S2−(aq)−→−CuS(s) Complete: Na+(aq)+OH−(aq)+HC2H3O2(aq)−→−H2O(l)+Na+(aq)+C2H3O−2(aq) Net: OH−(aq)+HC2H3O2(aq)−→−H2O(l)+C2H3O−2(aq) Complete: 6 Na+(aq)+2PO43−(aq)+3 Ni2+(aq)+6 Cl−(aq)→ Ni3(PO4)2(s)+6 Na+(aq)+6 Cl−(aq) Net: 3 Ni2+(aq)+2 PO4−3(aq)−→−Ni3(PO4)2(s)
Which of these ions will spontaneously react with Ni(s) in solution? a. Cu2+(aq) b. Zn2+(aq) c. Mg2+(aq) d. K+(aq)
Cu2+(aq)
Suppose you wanted to cause Ni2+ ions to come out of solution as solid Ni. Which metal could you use to accomplish this?
Fe, Cr, Zn, Mn, Al, Mg, Na, Ca, K, Li
Predict the charges of the monoatomic ions formed by these main group elements: Al, S, N, Rb
Go to nearest noble gas, Al 3+, S 2-, N3-, Rb+
What is the net ionic equation for the reaction that occurs when you mix aqueous solutions of KOH and HNO3?
H+(aq) + OH−(aq) → H2O(l)
What is the structural formula for Water?
H-O-H
Write a balanced equation for the reaction of hydrogen gas with bromine gas.
H2(g)+Br2(g)−→−2 Hbr(g)
Sodium reacts with water according to the reaction: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) Identify the oxidizing agent.
H2O(l)
Complete and balance each acid-base equation. MISSED THIS? Read Section 5.7; Watch IWE 5.9 a.H2SO4(aq)+Ca(OH)2(aq) −→− b.HClO4(aq)+KOH(aq) −→− c.H2SO4(aq)+NaOH(aq) −→−
H2SO4(aq)+Ca(OH)2(aq)−→−2 H2O(l)+CaSO4(s) HClO4(aq)+KOH(aq)−→−H2O(l)+KClO4(aq) H2SO4(aq)+2NaOH(aq)−→−2H2O(l)+Na2SO4(aq)
Identify the product of the reaction between hydrogen gas and bromine.
HBr
What is the net ionic equation for the reaction that occurs when you mix aqueous solutions of KHCO3 and HC2H3O2
HCO3−(aq) + HC2H3O2(aq) → H2O(l) + CO2(g) + C2H3O2−(aq)
Write the formula for perchloric acid.
HClO4
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl−Cl−. Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations for the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
Hg22+(aq)+2 NO3−(aq)+2Na+(aq)+2Cl−(aq)→ Hg2Cl2(s)+2Na+(aq)+2NO3−(aq) Net:Hg22+(aq)+2 NO3−(aq)+2 Na+(aq)+2Cl−(aq)→Hg2Cl2(s)
Predict whether the compound is soluble or insoluble. PbCl2
Insoluble
Classify the substance as an atomic element, molecular element, molecular compound, or ionic compound: NaNO3
Ionic Compound
Classify the substance as an atomic element, molecular element, molecular compound, or ionic compound: NiCl2
Ionic Compound
Write an equation for the precipitation reaction that occurs (if any) when solutions of potassium carbonate and nickel(II) chloride are mixed.
K2CO3 + NiCl2 -> KCl + NiCO3 NiCO3 is insoluble. K2CO3(aq) + NiCl2(aq) -> 2KCl(aq) + NiCO3(s)
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write "NO REACTION." MISSED THIS? Read Section 5.5; Watch KCV 5.5, IWE 5.6 a.potassium carbonate and lead(II) nitrate b.lithium sulfate and lead(II) acetate c.copper(II) nitrate and magnesium sulfide d.strontium nitrate and potassium iodide
K2CO3(aq)+Pb(NO3)2(aq)−→−PbCO3(s)+2 KNO3(aq) Li2SO4(aq)+Pb(C2H3O2)2(aq)−→−PbSO4(s)+2 LiC2H3O2(aq) Cu(NO3)2(aq)+MgS(aq)−→−CuS(s)+Mg(NO3)2(aq) NO REACTION
Write the formula for the compound produced between potassium and sulfur
K2S
Name the compound PbCl4
Lead(IV) chloride
Hydrogen and oxygen form both water and hydrogen peroxide. The decomposition of a sample of water forms 0.125 g hydrogen to every 1.00 g oxygen. The decomposition of a sample of hydrogen peroxide forms 0.0625 g hydrogen to every 1.00 g oxygen. Show that these results are consistent with the law of multiple proportions.
Mass of hydrogen to 1 g of oxygen in water/mass of hydrogen to 1 g of oxygen in hydrogen peroxide =0.125/0.0625=2.00. The ratio of the mass of hydrogen from one compound to the mass of hydrogen in the other is equal to 2. This is a simple whole number and therefore consistent with the law of multiple proportions.
A 20.0-g sample of an element contains 4.95 × 1023 atoms. Identify the element.
Mg
Which metal in the activity series reduces Al3+ ions but not Na+ ions?
Mg
Use oxidation states to identify the element that is oxidized and the element that is reduced in the following redox reaction: Mg(s)+2 H2O(l) −→− Mg(OH)2(aq)+H2(g)
Mg oxidized, Hydrogen reduced
What is the formula for manganese(IV) oxide?
MnO2
Classify the substance as an atomic element, molecular element, molecular compound, or ionic compound: NO2
Molecular Compound
Name SO2
Molecular compound, sulfur dioxide
What's the difference between ionic and molecular compounds?
Molecular compounds contain highly directional covalent bonds, which result in the formation of molecules. Ionic compounds contain nondirectional ionic bonds, which result (in the solid state) in the formation of ionic lattices.
Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.
Molecular: HBr(aq)+KOH(aq)−→−H2O(l)+KBr(aq) Net ionic: H+(aq)+OH−(aq)→H2O(l)
A compound containing nitrogen and oxygen is decomposed in the laboratory. It produces 24.5 g nitrogen and 70.0 g oxygen. Calculate the empirical formula of the compound.
N2O5
Select the equation for the precipitation reaction that occurs (if any) when solutions of ammonium chloride and iron(III) nitrate mix.
NH4+Cl- + Fe(No3)3 -> NH4(NO3) + FeCl Neither of these insoluble, so no reaction
Complete and balance each equation. If no reaction occurs, write "NO REACTION." MISSED THIS? Read Section 5.5; Watch KCV 5.5, IWE 5.6 a.LiI(aq)+BaS(aq) −→ b.KCl(aq)+CaS(aq) −→ c.CrBr2(aq)+Na2CO3(aq) −→ d.NaOH(aq)+FeCl3(aq) −→−
NO REACTION NO REACTION CrBr2(aq)+Na2CO3(aq)−→−CrCO3(s)+2 NaBr(aq) 3 NaOH(aq)+FeCl3(aq)−→−Fe(OH)3(s)+3 NaCl(aq)
Write the balanced chemical equation for the reaction of aqueous sodium carbonate with aqueous copper(II) chloride to form solid copper(II) carbonate and aqueous sodium chloride.
Na2CO3(aq)+CuCl2(aq)−→−CuCO3(s)+2 NaCl(aq)
Write an equation for the precipitation reaction that occurs (if any) when solutions of sodium nitrate and lithium sulfate are mixed.
NaNO3 + Li2SO4 -> Na2SO4 + LiNO3 Neither are insoluble. No reaction takes place.
P or C? Dry ice sublimes without melting
P
P or C? Evaporation of rubbing alcohol
P
Write the formula for phosphorus tribromide.
PBr3
Write a balanced equation for the reaction between aqueous lead(II) nitrate and aqueous potassium chloride to form solid lead(II) chloride and aqueous potassium nitrate.
Pb(NO3)2(aq)+2 KCl(aq)→PbCl2(s)+2 KNO3(aq)
Name the compound: PCl5
Phosphorous pentachloride
What type of energy is chemical energy?
Potential
Complete and balance each combustion reaction equation. MISSED THIS? Read Section 4.5 a.S(s) + O2(g) → b.C3H6(g) + O2(g) → c.Ca(s) + O2(g) → d.C5H12S(l) + O2(g) →
S(s)+O2(g)−→−SO2(g) 2 C3H6(g)+9 O2(g)−→−6 CO2(g)+6 H2O(g) 2 Ca(s)+O2(g)−→−2 CaO(g) C5H12S(l)+9 O2(g)−→−5 CO2(g)+SO2(g)+6 H2O(g)
The density of copper decreases as temperature increases (as does the density of most substances). Which change occurs in a sample of copper when it is warmed from room temperature to 95 °C?
Sample expands
Write a balanced equation for the reaction between solid silicon dioxide and solid carbon to produce solid silicon carbide and carbon monoxide gas.
SiO2(s)+3 C(s)→SiC(s)+2 CO(g)
The compound NCl3 is nitrogen trichloride, but AlCl3 is simply aluminum chloride. Why?
The name forms differ because NCl3 is a molecular compound and AlCl3 is an ionic compound. Prefixes such as mono-, di-, tri- are used for molecular compounds but not for ionic compounds.
Classify each hydrocarbon as an alkane, alkene, or alkyne. MISSED THIS? Read Section 3.11 a.H2C=CH—CH3H2C=CH—CH3 b.H3C—CH2—CH3 c.HC≡C—CH3HC≡C—CH3 d.H3C—CH2—CH2—CH3
alkene alkane alkyne alkane
Determine whether each redox reaction occurs spontaneously in the forward direction. MISSED THIS? Read Section 5.9 a.Ni(s)+Zn2+(aq) −→− Ni2+(aq)+Zn(s) b.Ni(s)+Pb2+(aq) −→− Ni2+(aq)+Pb(s) c.Al(s)+3 Ag+(aq) −→− Al3+(aq)+3 Ag(s) d.Pb(s)+Mn2+(aq) −→− Pb2+(aq)+Mn(s)
b and c occur spontaneously in the forward direction.
a.the tendency of ethyl alcohol to burn b.the shine on silver c.the odor of paint thinner d.the flammability of propane gas
chemical physical physical chemical
Natural gas burns in a stove. b.The liquid propane in a gas grill evaporates because the valve was left open. c.The liquid propane in a gas grill burns in a flame. d.A bicycle frame rusts on repeated exposure to air and water.
chemical, physical, chemical, chemical
Name the compound N2O5.
dinitrogen pentoxide
Name the compound P2I4
diphosphorous tetraiodide
Predict whether each compound is soluble or insoluble. BaSO4
insoluble
What are the atomic number, mass number, and symbol of chlorine isotope with 18 neutrons
mass number: 35, atomic number: 17, Cl
Classify each of the substances as an atomic element, molecular element, molecular compound, or ionic compound. fluorine N2O silver K2O Fe2O3
molecular element molecular compound atomic element ionic compound ionic compound
Name HNO3(aq)
nitric acid
Name the acid HNO2(aq).
nitrous acid
Name the compound HNO2(aq)
nitrous acid
Predict whether each compound is soluble or insoluble. CuCl2
soluble
Which quantity or quantities must always be the same on both sides of a chemical equation?
the number of atoms of each kind
A chromium-containing compound has the formula FexCryO4 and is 28.59% oxygen by mass. Find x and y.
x=1,y=2
For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? MISSED THIS? Read Section 5.4 a.CsCl b.CH3OH c.Ca(NO2)2 d.C6H12O6
yes no yes no
