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Chemistry
Q:
When Na2CrO4(aq) and AgNO3(aq) are mixed, a red colored precipitate forms which is
A) Ag.
B) Ag2CrO4.
C) AgNO2.
D) NaNO3.
Q:
When K2SO4(aq) and Pb(NO3)2(aq) are mixed, a white colored precipitate forms which is
A) KNO3.
B) K2SO3.
C) Pb.
D) PbSO4.
Q:
Which pair of reactants will produce a precipitate when mixed together?
A) HCl(aq) and NaOH(aq)
B) HCl(aq) and Na2CO3(aq)
C) HCl(aq) and Na2S(aq)
D) HCl(aq) and Pb(NO3)2(aq)
Q:
Predict the products of a reaction between Ba(NO3)2(aq) and K2SO4(aq).
A) Ba(s), KNO3(aq) and K2SO3(aq)
B) BaSO3(s) and KNO2(aq)
C) BaSO3(s) and KNO3(aq)
D) BaSO4(s) and KNO3(aq)
Q:
Predict the products of a reaction between AgNO3(aq) and KBr(aq).
A) Ag(s) and NO(g)
B) Ag(s) and Br2(l)
C) AgBr(s) and KNO3(aq)
D) AgNO3(aq) and KBr(aq)
Q:
What reagent could not be used to separate Cl- from OH- when added to an aqueous solution containing both?
A) AgNO3(aq)
B) Ca(NO3)2(aq)
C) Cu(NO3)2(aq)
D) Fe(NO3)3(aq)
Q:
What reagent could be used to separate Br- from NO3- when added to an aqueous solution containing both?
A) AgNO3(aq)
B) Ba(OH)2(aq)
C) CuSO4(aq)
D) NaI(aq)
Q:
The mixing of which pair of reactants will result in a precipitation reaction?
A) Cu(NO3)2(aq) + Na2CO3(aq)
B) K2SO4(aq) + Cu(NO3)2(aq)
C) NaClO4(aq) + (NH4)2S(aq)
D) NH4Br(aq) + NaI(aq)
Q:
The mixing of which pair of reactants will result in a precipitation reaction?
A) CsI(aq) + NaOH(aq)
B) HCl(aq) + Ca(OH)2(aq)
C) K2SO4(aq) + Ba(NO3)2(aq)
D) NaNO3(aq) + NH4Cl(aq)
Q:
Phthalic acid is a diprotic acid having the formula HO2CC6H4CO2H that can be converted to a salt by reaction with base. Which of the following is expected to be most soluble in water?
A) HO2CC6H4CO2H
B) HO2CC6H4CO2Na
C) HO2CC6H4CO2K
D) NaO2CC6H4CO2K
Q:
Which pair of compounds is soluble in water?
A) AgBr and AgI
B) CdS and (NH4)2S
C) KI and Ba(NO3)2
D) NaNO3 and CuCO3
Q:
Which one of the following compounds is soluble in water?
A) Ag3PO4
B) CuS
C) Pb(NO3)2
D) ZnCO3
Q:
Which pair of compounds is insoluble in water?
A) AgNO3 and KNO3
B) Na2S and CuS
C) (NH4)2SO4 and AgI
D) PbSO4 and Pb3(PO4)2
Q:
Which one of the following compounds is insoluble in water?
A) K2SO4
B) NaNO3
C) PbSO4
D) Rb2CO3
Q:
In the reaction AgNO3(aq) + HI(aq) -> AgI(s) + HNO3(aq) the spectator ions areA) Ag+ and NO3"B) Ag+ and I"C) H+ and I"D) H+ and NO3"
Q:
a balanced net ionic equation for the reaction of NiBr2(aq) with (NH4)2S(aq).A) NiBr2(aq) + (NH4)2S(aq) -> NiS(s) + 2 NH4Br(aq)B) Ni2+(aq) + 2 Br-(aq) + 2 NH4+(aq) + S2-(aq) -> NiS(s) + 2 NH4+(aq) + 2 Br-(aq)C) Ni2+(aq) + 2 Br-(aq) + 2 NH4+(aq) + S2-(aq) -> NiS(s) + 2 NH4Br(s)D) Ni2+(aq) + S2-(aq) -> NiS(s)
Q:
a balanced net ionic equation for the reaction of CdCl2(aq) with Na2S(aq).A) CdCl2(aq) + Na2S(aq) -> CdS (aq) + 2 NaCl(aq)B) Cd2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + S2-(aq) -> CdS(s) + 2 NaCl(aq)C) Cd2+(aq) + S2-(aq) -> CdS(s)D) Cd2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + S2-(aq) -> CdS(s) + 2 Na+(aq)
Q:
a balanced net ionic equation for the reaction of AgNO3(aq) with KBr(aq).A) AgNO3(aq) + KBr(aq) -> AgBr(aq) + KNO3(s)B) Ag+(aq) + NO3-(aq) + K+(aq) + Br-(aq) -> Ag+(aq) + Br-(aq) + KNO3(s)C) Ag+(aq) + NO3-(aq) + K+(aq) + Br-(aq) -> AgBr(s) + K+(aq) + NO3-(aq)D) Ag+(aq) + Br-(aq) -> AgBr(s)
Q:
a balanced net ionic equation for the reaction of AgNO3(aq) with Cu(s).A) AgNO3(aq) + Cu(s) -> Ag(s) + CuNO3(aq)B) Ag+(aq) + Cu(s) -> Ag(s) + Cu+(aq)C) 2 AgNO3(aq) + Cu(s) -> 2 Ag(s) + CuNO3(aq)D) 2Ag+(aq) + Cu(s) -> 2 Ag(s) + Cu2+(aq)
Q:
a balanced net ionic equation for the reaction of Na2CO3(s) and HCl(aq).A) Na2CO3(s) + 2 HCl(aq) -> 2 NaCl(aq) + H2O(l) + CO2(g)B) 2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) -> 2Na+(aq) + 2Cl-(aq) + H2O(l) + CO2(g)C) Na2CO3(s) + 2 H+(aq) -> 2 Na+(aq) + H2O(l) + CO2(g)D) CO32-(aq) + 2 H+(aq) -> H2O(l) + CO2(g)
Q:
a balanced net ionic equation for the reaction of H2SO4(aq) with Ba(OH)2(aq).A) H2SO4(aq) + Ba(OH)2(aq) -> BaSO4(s) + 2 H2O(l)B) 2 H+(aq) + SO42-(aq) + Ba2+(aq) + 2 OH-(aq) -> BaSO4(s) + 2 H2O(l)C) H+(aq) + OH+(aq) -> H2O(l)D) Ba2+(aq) + SO42-(aq) -> BaSO4(s)
Q:
a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq).A) Pb(NO3)2(aq) + 2 NaI(aq) -> PbI2(s) + 2 NaNO3(aq)B) Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) -> Pb2+(aq) + 2 I-(aq) + 2 Na+(aq) + 2 NO3-(aq)C) Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) -> PbI2(s) + 2 Na+(aq) + 2 NO3-(aq)D) Pb2+(aq) + 2 I-(aq) -> PbI2(s)
Q:
What is the molar concentration of sulfate ions in a 0.150 M Na2SO4 solution?
A) 0.075 M
B) 0.150 M
C) 0.300 M
D) 0.450 M
Q:
What is the molar concentration of sodium ions in a 0.350 M Na3PO4 solution?
A) 0.117 M
B) 0.350 M
C) 1.05 M
D) 1.40 M
Q:
In a solution prepared by mixing CH3OH with H2O the major species present areA) CH3OH and H2OB) CH3OH, H+, and OH"C) CH3+, OH", and H2OD) CH3O-, H+, and H2O
Q:
Water (H2O), methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH), ethylene glycol (HOCH2CH2OH), and sucrose (C12H22O11) are commonly classified as
A) bases.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
Q:
Acetic acid (CH3CO2H), formic acid (HCO2H), hydrofluoric acid (HF), aqueous ammonia (NH3), and aqueous methylamine (CH3NH2) are commonly classified as
A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
Q:
HBr, HCl, HClO4, KBr, and NaCl are all classified as
A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
Q:
The combustion reaction CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) can be classified as a(n)A) acid-base neutralization reaction.B) double replacement reaction.C) oxidation-reduction reaction.D) precipitation reaction.
Q:
The reaction C6H12O6(s) + 6 O2(g) -> 6 CO2(g) + 6 H2O(l) is best classified as a(n)A) acid-base neutralization reaction.B) double replacement reaction.C) oxidation-reduction reaction.D) precipitation reaction.
Q:
The reaction Cu(s) + 2 AgNO3(aq) -> Cu(NO3)2(aq) + 2 Ag(s) is best classified as a(n)A) acid-base neutralization reaction.B) double replacement reaction.C) oxidation-reduction reaction.D) precipitation reaction.
Q:
The reaction Na3PO4(aq) + 3 AgNO3(aq) -> Ag3PO4(s) + 3 NaNO3(aq) is best classified as a(n)A) acid-base neutralization reaction.B) oxidation-reduction reaction.C) precipitation reaction.D) single replacement reaction.
Q:
The reaction Pb(NO3)2(aq) + K2SO4(aq) -> PbSO4(s) + 2 KNO3(aq) is best classified as a(n)A) acid-base neutralization reaction.B) oxidation-reduction reaction.C) precipitation reaction.D) single replacement reaction.
Q:
The reaction 2 HNO3(aq) + Ba(OH)2(aq) -> Ba(NO3)2(aq) + 2 H2O(l) is best classified as a(n)A) acid-base neutralization reaction.B) oxidation-reduction reaction.C) precipitation reaction.D) single replacement reaction.
Q:
The reaction HNO3(aq) + KOH(aq) -> KNO3(aq) + H2O(l) is best classified as a(n)A) acid-base neutralization reaction.B) oxidation-reduction reaction.C) precipitation reaction.D) single replacement reaction.
Q:
What is the concentration of an AlCl3 solution if 150. mL of the solution contains 450. mg of Cl- ion?
A) 2.82 10-2 M
B) 6.75 10-2 M
C) 8.46 10-2 M
D) 2.54 10-1 M
Q:
What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?
A) 0.254 M
B) 0.508 M
C) 0.672 M
D) 1.02 M
Q:
What volume of a 0.540 M NaOH solution contains 11.5 g of NaOH?
A) 0.155 L
B) 0.532 L
C) 1.88 L
D) 6.44 L
Q:
What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough water to make 275 mL of solution?
A) 4.48 10-4 M
B) 0.448 M
C) 2.23 M
D) 2.23 103 M
Q:
Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25C? The density of nitrogen monoxide at 25C is 1.23 g/L.________ NH3(g) + ________ O2(g) -> ________ NO(g) + ________ H2O(l)A) 11.2 LB) 16.1 LC) 11.5 LD) 17.3 L
Q:
When 7.00 1022 molecules of ammonia react with 6.00 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced?4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(g)A) 1.63 gB) 1.86 gC) 4.19 gD) 6.51 g
Q:
7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is false?N2(g) + 3 H2(g) -> 2 NH3(g)A) 3.5 g of hydrogen are left over.B) Hydrogen is the excess reactant.C) Nitrogen is the limiting reactant.D) The theoretical yield of ammonia is 15 g.
Q:
If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 32.0 g of O2?2 KClO3(s) -> 2 KCl(s) + 3 O2(g)A) 53.1 gB) 81.7 gC) 126 gD) 283 g
Q:
When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction?Ca(s) + 2 H2O(l) -> Ca(OH)2(aq) + H2(g)A) 12.3%B) 24.6%C) 45.5%D) 84.0%
Q:
If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation?C2H5OH(l) + 3 O2(g) -> 2 CO2(g) + 3 H2O(l)A) 6.19 mLB) 9.95 mLC) 19.9 mLD) 39.8 mL
Q:
Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?
A) 0.275 g
B) 3.64 g
C) 7.27 g
D) 14.5 g
Q:
Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3 .________ MgO(s) + ________ Fe(s) -> ________ Fe2O3(s) + ________ Mg(s)A) 0.312 gB) 0.841 gC) 2.52 gD) 7.57 g
Q:
Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum.________ Al(s) + ________ I2(s) -> ________ Al2I6(s)A) 0.741 molB) 1.67 molC) 2.22 molD) 3.33 mol
Q:
How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?CaCl2(aq) + K2CO3(aq) -> 2 KCl(aq) + CaCO3(aq)A) 0.896 gB) 1.12 gC) 2.23 gD) 4.47 g
Q:
How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction?BCl3(g) + 3 H2O(l) -> 3 HCl(aq) + B(OH)3(aq)A) 0.0914 molB) 0.274 molC) 0.823 molD) 10.9 mol
Q:
How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction?2 Cu2O(s) + O2(g) -> 4 CuO(s)A) 0.450 molB) 0.900 molC) 1.80 molD) 3.60 mol
Q:
Which of the following has the greatest mass?
A) 3.88 1022 molecules of O2
B) 1.00 g of O2
C) 0.0312 mol of O2
D) All of the above have the same mass.
Q:
How many cations are there in 10.0 g of sodium phosphate?
A) 3.67 1022 cations
B) 1.10 1023 cations
C) 9.87 1024 cations
D) 2.96 1025 cations
Q:
How many anions are there in 2.50 g of MgBr2?
A) 8.18 1021 anions
B) 1.64 1022 anions
C) 4.43 1025 anions
D) 8.87 1025 anions
Q:
What mass of phosphorus pentafluoride, PF5, has the same number of fluorine atoms as 25.0 g of oxygen difluoride, OF2?
A) 0.933 g
B) 10.0 g
C) 23.3 g
D) 146 g
Q:
What mass of carbon dioxide, CO2, contains the same number of molecules as 3.00 g of trichlorofluoromethane, CCl3F?
A) 0.106 g
B) 0.961 g
C) 1.04 g
D) 9.37 g
Q:
What is the molar mass of 1-butene if 5.38 1016 molecules of 1-butene weigh 5.00 μg?
A) 56.0 g/mol
B) 178 g/mol
C) 224 g/mol
D) 447 g/mol
Q:
How many chloride ions are there in 4.50 mol of aluminum chloride?
A) 3.00 chloride ions
B) 13.5 chloride ions
C) 2.71 1024 chloride ions
D) 8.13 1024 chloride ions
Q:
How many oxygen atoms are there in 7.00 g of sodium dichromate, Na2Cr2O7?
A) 0.187 oxygen atoms
B) 2.30 1021 oxygen atoms
C) 1.60 1022 oxygen atoms
D) 1.13 1023 oxygen atoms
Q:
What is the mass of 8.50 x 1022 molecules of NH3?
A) 0.00829 g
B) 0.417 g
C) 2.40 g
D) 121 g
Q:
How many Fe(II) ions are there in 20.0 g of FeSO4?
A) 2.19 10-25 iron(II) ions
B) 7.92 1022 iron(II) ions
C) 4.57 1024 iron(II) ions
D) 1.82 1027 iron(II) ions
Q:
How many moles are there in 3.00 g of ethanol, CH3CH2OH?
A) 0.00725 mol
B) 0.0652 mol
C) 15.3 mol
D) 138 mol
Q:
What is the mass of 0.500 mol of dichlorodifluoromethane, CCl2F2?
A) 4.14 10-3 g
B) 60.5 g
C) 121 g
D) 242 g
Q:
What is the mass of a single fluorine molecule, F2?
A) 3.155 10-23 g
B) 6.310 10-23 g
C) 19.00 g
D) 38.00 g
Q:
What is the molar mass of nitrogen gas?
A) 14.0 g/mol
B) 28.0 g/mol
C) 6.02 1023 g/mol
D) 1.20 1023 g/mol
Q:
Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered coefficients?
A) 1
B) 2
C) 3
D) none of these
Q:
Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?
A) 1
B) 2
C) 3
D) 4
Q:
What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients?________ C2H6O(l) + ________ O2(g) -> ________ CO2(g) + ________ H2O(l)A) 9B) 7C) 5D) 3
Q:
A hydrocarbon of unknown formula CxHy was submitted to combustion analysis with the following results. What is the empirical formula of the hydrocarbon?A) C5H2B) C5H4C) C10H4D) C10H8
Q:
A hydrocarbon of unknown formula CxHy was submitted to combustion analysis with the following results. What is the empirical formula of the hydrocarbon? A) CH
B) C2H
C) C2H4
D) C4H4
Q:
Glucose, C6H1206, can be represented by the molecular model shown below. If 1.00 mol of glucose is submitted to combustion analysis, how many moles of CO2 and how many moles of H2O would be formed? A) 1.00 mol CO2 and 2.00 mol H2O
B) 6.00 mol CO2 and 6.00 mol H2O
C) 6.00 mol CO2 and 12.0 mol H2O
D) 12.0 mol CO2 and 12.0 mol H2O
Q:
Ascorbic acid, C6H806, can be represented by the molecular model shown below. If 1.00 mol of ascorbic acid is submitted to combustion analysis, how many moles of CO2 and how many moles of H2O would be formed? A) 3.00 mol CO2 and 2.00 mol H2O
B) 6.00 mol CO2 and 4.00 mol H2O
C) 6.00 mol CO2 and 8.00 mol H2O
D) 12.0 mol CO2 and 10.0 mol H2O
Q:
If the volumes in the buret and the flask are identical and the concentration of the acid in the buret is 0.500 M, what is the concentration of the base in the flask?
A) 0.333 M
B) 0.500 M
C) 0.667 M
D) 0.750 M
Q:
Assume that the unshaded spheres in the buret represent H+ ions, the shaded spheres in the flask represent OH- ions, and you are carrying out a titration of the base with the acid.If the volumes in the buret and the flask are identical and the concentration of the acid in the buret is 0.250 M, what is the concentration of the base in the flask?A) 0.167 MB) 0.250 MC) 0.375 MD) 0.667 M
Q:
Which of the boxes (2)-(5) represents 1.0 mL of the solution that results after (1) has been diluted by adding enough solvent to make 5.0 mL of solution?A) box (2)B) box (3)C) box (4)D) box (5)
Q:
Box (1) represents 1.0 mL of a solution of particles at a given concentration.Which of the boxes (2)-(5) represents 1.0 mL of the solution that results after (1) has been diluted by adding enough solvent to make 2.0 mL of solution?A) box (2)B) box (3)C) box (4)D) box (5)
Q:
The following diagrams represent the reaction of A2 (shaded spheres) with B2 (unshaded spheres). How many moles of product can be made from 1.0 mol of A2 and 1.0 mol of B2?A) 0.67 mol productB) 1.0 mol productC) 2.0 mol productD) 3.0 mol product
Q:
The following diagram represents the reaction of A2 (unshaded spheres) with B2 (shaded spheres). How many moles of product can be produced from the reaction of 1.0 mol of A2 and 1.0 mol of B2? A) 0.5 mol of product
B) 1.0 mol of product
C) 2.0 mol of product
D) 4.0 mol of product
Q:
The following diagram represents the reaction of A2 (unshaded spheres) with B (shaded spheres). How many moles of product can be produced from the reaction of 1.0 mol of A2 and 1.0 mol of B? A) 0.5 mol of product
B) 1.0 mol of product
C) 3.0 mol of product
D) 6.0 mol of product
Q:
The following diagrams represent the reaction of A2 (shaded spheres) with B2 (unshaded spheres). Identify the limiting reactant and a balanced equation for the reaction.A) A2 is the limiting reactant; A + 3 B -> AB3.B) A2 is the limiting reactant; A2 + 3 B2 -> 2 AB3.C) B2 is the limiting reactant; A + 3 B -> AB3.D) B2 is the limiting reactant; A2 + 3 B2 -> 2 AB3.