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Chemistry
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 + 4 B -> AB4.B) A2 is the limiting reactant; A2 + 4 B2 -> 2 AB4.C) B2 is the limiting reactant; A + 4 B -> AB4.D) B2 is the limiting reactant; A2 + 4 B2 -> 2 AB4.
Q:
The following diagram represents the reaction of A2 (unshaded spheres) with B (shaded spheres). What is the balanced chemical equation for this reaction, and what is the limiting reactant?A) 2A2 + B -> A4B; A2 is the limiting reactant.B) 2A2 + B -> A4B; B is the limiting reactant.C) 4A2 + 6B -> 2A4B; A2 is the limiting reactant.D) 4A2 + 6B -> 2A4B; B is the limiting reactant.
Q:
The following diagram represents the reaction of A2 (unshaded spheres) with B (shaded spheres). What is the balanced chemical equation for this reaction, and what is the limiting reactant?A) A2 + 2B -> 2AB; A2 is the limiting reactant.B) A2 + 2B -> 2AB; B is the limiting reactant.C) 4A2 + 6B -> 6AB; A2 is the limiting reactant.D) 4A2 + 6B -> 6AB; B is the limiting reactant.
Q:
Reaction of A (unshaded spheres) with B2 (shaded spheres) is shown schematically in the following diagram. Which equation best describes the stoichiometry of the reaction?A) 4 A + B2 -> 8 A2BB) 4 A + B2 -> A4B2C) 16 A + 4 B2 -> 8 A2BD) 16 A + 4 B2 -> 4 A4B2
Q:
Reaction of A (unshaded spheres) with B2 (shaded spheres) is shown schematically in the following diagram. Which equation best describes the stoichiometry of the reaction?A) A2 + 2 B -> A2B2B) 8 A + 4 B2 -> 4 A2B2C) 2 A + B2 -> A2B2D) 4 A + 4 B2 -> 4 A2B2
Q:
What is the balanced chemical equation for the reaction of element A (unshaded spheres) with element B (shaded spheres) as represented below?A) A + B -> ABB) 2A + 3B -> 2ABC) A + B2 -> AB3D) 2A + 3B2 -> 2AB3
Q:
What is the balanced chemical equation for the reaction of element A (unshaded spheres) with element B (shaded spheres) as represented below?A) A + B -> ABB) A + 3B -> 2ABC) A2 + B2 -> AB3D) A2 + 3B2 -> 2AB3
Q:
What is the balanced chemical equation for the reaction of element A (unshaded spheres) with element B (shaded spheres) as represented below?A) A + B -> ABB) A + 3B -> 3ABC) A2 + B -> ABD) A2 + 2B -> 2AB
Q:
What is the balanced chemical equation for the reaction of element A (unshaded spheres) with element B (shaded spheres) as represented below?A) A + B -> ABB) 4A + 2B -> 4ABC) A2 + B2 -> A2BD) 2A2 + B2 -> 2A2B
Q:
3If unshaded spheres represent nitrogen atoms and shaded spheres represent oxygen atoms, which box represents reactants and which represents products for the reaction 2 N2O(g) → 2 N2(g) + O2(g)? A) box (a) reactants and box (c) products
B) box (a) reactants and box (d) products
C) box (b) reactants and box (c) products
D) box (b) reactants and box (d) products
Q:
If unshaded spheres represent nitrogen atoms and shaded spheres represent oxygen atoms, which box represents reactants and which represents products for the reaction 2 NO2(g) → 2 NO(g) + O2(g)? A) box (a) reactants and box (b) products
B) box (a) reactants and box (d) products
C) box (c) reactants and box (b) products
D) box (c) reactants and box (d) products
Q:
2-Propanol has the molecular formula C3H8O. Which ball and stick model shown above represents 2-propanol? [gray spheres = C, black spheres = O, unshaded spheres = H]
A) model a)
B) model b)
C) model c)
D) model d)
Q:
Ethanol has the molecular formula C2H6O. Which ball and stick model shown above represents ethanol? [gray spheres = C, black spheres = O, unshaded spheres = H]
A) model a)
B) model b)
C) model c)
D) model d)
Q:
Diethyl ether has the molecular formula C4H10O. Which ball and stick model shown above represents diethyl ether? [gray spheres = C, black spheres = O, unshaded spheres = H]
A) model a)
B) model b)
C) model c)
D) model d)
Q:
Acetone has the formula C3H6O. Which ball and stick model shown above represents acetone? [gray spheres = C, black spheres = O, unshaded spheres = H]A) model a)B) model b)C) model c)D) model d)
Q:
Which of the following statements about mass spectrometry is false?A) Mass spectrometry can be used to determine the molecular weight of a compound.B) The curvature of the path in a magnetic field is determined by the mass of the ion.C) The paths of heavier ions are deflected more strongly than the paths of lighter ions.D) The sample is changed into positively charged ions.
Q:
Molecular mass can be determined by
A) combustion analysis.
B) mass spectrometry.
C) titration.
D) weighing with an analytical balance.
Q:
Isoeugenol is the compound which gives the characteristic odor to nutmeg and contains carbon, hydrogen, and oxygen. If a 0.500 g sample of isoeugenol is combusted it gives 1.341 g of CO2 and 0.329 g of H2O. Isoeugenol has a molecular weight of 164 g/mol. What is the molecular formula of isoeugenol?
A) C2HO
B) C5H6O
C) C8H4O4
D) C10H12O2
Q:
Combustion analysis of a 0.675 g sample of an unknown compound that contains only carbon, hydrogen, and oxygen gives 0.627 g of CO2 and 1.534 g of H2O. The molecular mass of the unknown is
A) C3H6O.
B) C6H12O2.
C) C9H18O3.
D) unable to be determined from this data.
Q:
Combustion analysis of 2.400 g of an unknown compound containing carbon, hydrogen, and oxygen produced 4.171 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound?
A) C2H5O
B) C2H5O2
C) C2H10O3
D) C3H8O2
Q:
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 4.554 g of CO2 and 2.322 g of H2O. What is the empirical formula of the compound?
A) CH2
B) C2H5
C) C4H10
D) C5H2
Q:
In the combustion analysis of an unknown compound containing only carbon, hydrogen, and oxygen, the grams of oxygen are found from the grams of
A) CO2 only.
B) H2O only.
C) CO2 and H2O only.
D) CO2, H2O and unknown compound.
Q:
Which statement about elemental analysis by combustion is not correct?
A) Carbon is determined from the amount of CO2 formed.
B) Hydrogen is determined from the amount of H2O formed.
C) Oxygen is determined from the amount of H2O formed.
D) Only carbon and hydrogen can be determined directly from CO2 and H2O.
Q:
A compound responsible for the odor of garlic has a molecular weight of 146 g/mol. A 0.650 g sample of the compound contains 0.321 g of carbon, 0.044 g of hydrogen, and 0.285 g of sulfur. What is the molecular formula of the compound?
A) CH5S
B) C3H5S
C) C3H15S3
D) C6H10S2
Q:
Which one of the following is an empirical formula?
A) C2F6
B) H2SO4
C) N2H4
D) P4O10
Q:
What is the empirical formula for perfluoropropane if the compound contains 81% fluorine and 19% carbon by mass?
A) CF3
B) C2F8
C) C3F8
D) C19F81
Q:
What is the empirical formula for ethyl fluoride if the compound contains 49.97% carbon, 10.51% hydrogen, and 39.52% fluorine by mass?
A) C2H5F
B) C4H10F2
C) C4H10F4
D) C25F2
Q:
Which of the following statements is false concerning the formula of a compound?
A) The empirical formula is the simplest whole numbered ratio of atoms in a compound.
B) The molecular formula is the true ratio of atoms in a compound.
C) The molecular formula and empirical formula can be identical.
D) The number of atoms in a molecular formula is always greater than the number of atoms in an empirical formula.
Q:
Which one of the following contains 35% carbon by mass?
A) C2H2
B) CH4
C) CH3F
D) CO2
Q:
Which one of the following compounds contains the smallest percent oxygen by mass?
A) CO2
B) N2O4
C) P4O10
D) SO2
Q:
Balance the chemical equation given below, and determine the number of milliliters of 0.0300 M phosphoric acid required to neutralize 25.00 mL of 0.0150 M calcium hydroxide.___ Ca(OH)2(aq) + ___ H3PO4(aq) -> ___ Ca3(PO4)2(s) + ___ H2O(l)A) 1.69 mLB) 8.33 mLC) 12.5 mLD) 18.8 mL
Q:
In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?
A) 0.119 M
B) 0.237 M
C) 0.475 M
D) 2.11 M
Q:
How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH?HI(aq) + CsOH(aq) -> CsI(aq) + H2O(l)A) 0.0158 mLB) 0.101 mLC) 9.86 mLD) 63.4 mL
Q:
If 100. mL of 0.100 M Na2SO4 is added to 200. mL of 0.150 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.
A) 0.133 M
B) 0.167 M
C) 0.250 M
D) 0.350 M
Q:
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of Fe2S3 if the percent yield for the reaction is 65.0%?3 Na2S(aq) + 2 FeCl3(aq) -> Fe2S3(s) + 6 NaCl(aq)A) 50.9 mLB) 86.0 mLC) 102 mLD) 203 mL
Q:
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl, how many grams of AgCl are formed?AgNO3(aq) + NH4Cl(aq) -> AgCl(s) + NH4NO3(aq)A) 4.30 gB) 8.96 gC) 13.3 gD) 25.8 g
Q:
How many grams of CaCl2 are formed when 35.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas?2 Ca(OH)2(aq) + 2 Cl2(g) -> Ca(OCl)2(aq) + CaCl2(aq) + 2 H2O(l)A) 0.00460 gB) 0.00921 gC) 0.0184 gD) 0.0217 g
Q:
How many milliliters of 0.260 M Na2S are needed to react with 25.00 mL of 0.315 M AgNO3?Na2S(aq) + 2 AgNO3(aq) -> 2 NaNO3(aq) + Ag2S(s)A) 15.1 mLB) 30.3 mLC) 41.3 mLD) 60.6 mL
Q:
A student prepared a stock solution by dissolving 20.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?
A) 0.548 M
B) 0.713 M
C) 1.40 M
D) 1.82 M
Q:
A student dissolved 3.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the solution then diluted it with water to give 275 mL of a final solution. How many grams of NO3- ion are there in the final solution?
A) 0.0148 g
B) 0.0296 g
C) 0.0407 g
D) 0.0813 g
Q:
How many mL of a 0.175 M FeCl3 solution are needed to make 250. mL of a solution that is 0.300 M in Cl- ion?
A) 0.429 mL
B) 143 mL
C) 429 mL
D) It is not possible to make a more concentrated solution from a less concentrated solution.
Q:
How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.25 L of a 3.5 M H2SO4 solution?
A) 0.097 mL
B) 0.64 mL
C) 97 mL
D) 640 mL
Q:
What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L?
A) 2.8 10-2 M
B) 5.2 M
C) 28 M
D) 5.2 103 M
Q:
Which statement about diluted solutions is false? When a solution is diluted
A) the concentration of the solution decreases.
B) the molarity of the solution decreases.
C) the number of moles of solute remains unchanged.
D) the number of moles of solvent remains unchanged.
Q:
When a 1.0 M solution of NaCl at 25C is heated to 55C, the
A) density decreases and the molarity decreases.
B) density decreases and the molarity increases.
C) density increases and the molarity decreases.
D) density increases and the molarity increases.
Q:
Which contains the greatest number of chloride ions?
A) 25 mL of 2.0 M NaCl
B) 50 mL of 1.0 M CaCl2
C) 10 mL of 2.5 M FeCl3
D) All contain the same number of chloride ions.
Q:
What is the concentration of an AlCl3 solution if 150. mL of the solution contains 250. mg of Cl- ion?
A) 1.57 10-2 M
B) 3.75 10-2 M
C) 4.70 10-2 M
D) 1.41 10-1 M
Q:
If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?
A) 0.0101 M
B) 0.0404 M
C) 0.162 M
D) 0.323 M
Q:
What is the concentration of NO3- ions in a solution prepared by dissolving 15.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?
A) 0.152 M
B) 0.305 M
C) 0.403 M
D) 0.609 M
Q:
What volume of a 0.540 M NaOH solution contains 15.5 g of NaOH?
A) 0.209 L
B) 0.718 L
C) 1.39 L
D) 4.78 L
Q:
How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 M?
A) 0.0917 g
B) 0.174 g
C) 5.73 g
D) 91.7 g
Q:
What is the concentration of FeCl3 in a solution prepared by dissolving 10.0 g of FeCl3 in enough water to make 275 mL of solution?
A) 2.24 10-4 M
B) 0.224 M
C) 4.46 M
D) 4.46 103 M
Q:
Molarity is defined as
A) moles of solute per liter of solution.
B) moles of solute per liter of solvent.
C) moles of solvent per liter of solution.
D) moles of solvent per liter of solvent.
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) 7.32 LB) 11.2 LC) 16.5 LD) 18.8 L
Q:
When iron(III) oxide reacts with hydrochloric acid, iron(III) chloride and water are formed. How many grams of iron(III) chloride are formed from 10.0 g of iron(III) oxide and 10.0 g of hydrochloric acid?
A) 11.1 g
B) 14.8 g
C) 20.3 g
D) 35.1 g
Q:
When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride?
A) 8.44 g
B) 9.40 g
C) 11.9 g
D) 18.8 g
Q:
How many grams of the excess reagent are left over when 6.00 g of CS2 gas react with 10.0 g of Cl2 gas in the following reaction:CS2(g) + 3 Cl2(g) -> CCl4(l) + S2Cl2(l)A) 2.42 gB) 2.77 gC) 3.58 gD) 4.00 g
Q:
When 5.00 1022 molecules of ammonia react with 4.00 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) 1.16 gB) 1.24 gC) 2.79 gD) 4.65 g
Q:
Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation:2 S(s) + 3 O2(g) + 4 NaOH(aq) -> 2 Na2SO4(aq) + 2 H2O(l)A) S(s)B) O2(g)C) NaOH(aq)D) None of these substances is the limiting reactant.
Q:
5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which one of the following statements is false?3 Fe(s) + 4 H2O(l) -> Fe3O4(s) + 4 H2(g)A) 6.91 g of Fe3O4 are produced.B) 2.85 g of H2O are left over.C) Mass is conserved in this reaction.D) Water is the limiting reactant.
Q:
10 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) 2.8 grams 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:
When methane, CH4, undergoes combustion with oxygen, the usual products are carbon dioxide and water. Carbon monoxide is formed when the limiting reactant is
A) carbon dioxide.
B) methane.
C) oxygen.
D) water.
Q:
In the reaction between glucose and oxygen, 10.0 g of glucose reacts and 7.50 L of carbon dioxide is formed. What is the percent yield if the density of CO2 is 1.26 g/L?C6H12O6(s) + 6 O2(g) -> 6 CO2(g) + 6 H2O(l)A) 26.1%B) 40.6%C) 43.1%D) 64.5%
Q:
If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced?3 NO2(g) + H2O(l) -> 2 HNO3(aq) + NO(g)A) 30.8 gB) 41.1 gC) 54.8 gD) 69.3 g
Q:
If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 42.0 g of O2?2 KClO3(s) -> 2 KCl(s) + 3 O2(g)A) 69.7 gB) 107 gC) 165 gD) 371 g
Q:
When 10.0 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) 13.5%B) 27.1%C) 50.0%D) 92.4%
Q:
The density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 10.0 g of CO2 according to the following chemical equation?C2H5OH(l) + 3 O2(g) -> 2 CO2(g) + 3 H2O(l)A) 4.12 mLB) 6.63 mLC) 13.2 mLD) 26.5 mL
Q:
Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 5.00 g of dinitrogen monoxide decomposes?
A) 0.550 g
B) 1.82 g
C) 3.64 g
D) 7.27 g
Q:
Balance the chemical equation given below, and determine the number of grams of MgO needed to produce 15.0 g of Fe2O3.___ MgO(s) + ___ Fe(s) -> ___ Fe2O3(s) + ___ Mg(s)A) 0.0877 gB) 1.26 gC) 3.78 gD) 11.4 g
Q:
Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 10.0 g of aluminum.___ Al(s) + ___ I2(s) -> ___ Al2I6(s)A) 0.247 molB) 0.556 molC) 0.741 molD) 1.11 mol
Q:
How many grams of calcium chloride are needed to produce 10.0 g of potassium chloride?CaCl2(aq) + K2CO3(aq) -> 2 KCl(aq) + CaCO3(aq)A) 0.134 gB) 7.44 gC) 14.9 gD) 29.8 g
Q:
How many moles of BCl3 are needed to produce 25.0 g of HCl(aq) in the following reaction?BCl3(g) + 3 H2O(l) -> 3 HCl(aq) + B(OH)3(aq)A) 0.229 molB) 0.686 molC) 2.06 molD) 4.38 mol
Q:
How many moles of CuO can be produced from 0.450 mol of Cu2O in the following reaction?2 Cu2O(s) + O2(g) -> 4 CuO(s)A) 0.225 molB) 0.450 molC) 0.900 molD) 1.80 mol
Q:
Which of the following has the smallest mass?
A) 3.50 1023 molecules of I2
B) 85.0 g of Cl2
C) 2.50 mol of F2
D) 0.050 kg of Br2
Q:
Which of the following has the greatest mass?
A) 6.02 1023 molecules of O2
B) 16.0 g of O2
C) 0.500 mol of O2
D) All of the above have the same mass.
Q:
Which of the following has the greatest mass?
A) 6.0 1023 atoms of O
B) 3.0 1023 molecules of O2
C) 2.0 1023 molecules of O3
D) All have the same mass.
Q:
How many cations are 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 in 0.500 g of MgBr2?
A) 1.64 1021 anions
B) 3.27 1021 anions
C) 2.22 1026 anions
D) 4.43 1026 anions
Q:
How many chloride ions are in 1.50 mol of aluminum chloride?
A) 3.00 chloride ions
B) 4.50 chloride ions
C) 9.03 1023 chloride ions
D) 2.71 1024 chloride ions
Q:
What mass of sulfur hexafluoride, SF6, has the same number of fluorine atoms as 25.0 g of oxygen difluoride, OF2?
A) 0.901 g
B) 8.33 g
C) 22.5 g
D) 203 g