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Chemistry
Q:
Ozone reacts with iodide ion as shown in the balanced equation below.O3 + 2 I- + H2O -> O2 + I2 + 2 OH-In this reaction, how many grams of dioxygen can be formed from the reaction of 96 grams of ozone?
Q:
If 4.0 g of H2 react with 4.0 g of F2 in the reaction shown below, what is the limiting reactant?H2 + F2 -> 2 HF
Q:
Oxygen can be produced from the catalytic decomposition of KClO3 as shown in the balanced equation below.2 KClO3 -> 2 KCl + 3 O2What is the percent yield if 3.20 grams of oxygen are formed from the reaction of 12.3 grams of KClO3?
Q:
The balanced equation for the decomposition of water is shown below.2 H2O -> 2 H2 + O2If 0.72 g of water react completely in this reaction, what is the theoretical yield of H2?
Q:
Ozone is unstable, decomposing to dioxygen, as shown in the balanced equation2 O3 -> 3 O2.In this reaction, how many grams of dioxygen can be formed from the decomposition of 96 grams of ozone?
Q:
The balanced equation for the reaction of acetylene, C2H2, and oxygen in an acetylene torch is2 C2H2 + 5 O2 -> 4 CO2 + 2 H2O.In this reaction the number of grams of oxygen required to react with 0.13 g of acetylene is ________.
Q:
How many moles are in 7.8 g of acetamide, CH3CONH2?
Q:
The number of grams in 0.333 mol of urea, (NH2)2CO, is ________.
Q:
To the nearest whole number, the molar mass of Cu(NO3)2 is ________ g/mol.
Q:
The fundamental SI unit for measuring matter is the ________.
Q:
When the reaction C3H8 + O2 -> CO2 + H2O is balanced, the total number of oxygen atoms in the balanced equation is ________.
Q:
When the reaction C4H10 + O2 -> CO2 + H2O is balanced using the smallest whole number coefficients, the coefficient in front of O2 is ________.
Q:
A balanced equation has the same numbers and kinds of ________ on both sides of the reaction arrow.
Q:
Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?A) C2H5OB) C2H5O2C) C2H10O3D) C3H8O2
Q:
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 0.2845 g of CO2 and 0.1451 g of H2O. What is the empirical formula of the compound?
A) CH2
B) C4H5
C) C4H10
D) C5H2
Q:
Which one of the following contains 39% carbon by mass?
A) C2H2
B) CH4
C) CH3NH2
D) CO2
Q:
When 280. mL of 1.50 10-4 M hydrochloric acid is added to 125 mL of 1.75 10-4 M Mg(OH)2, the resulting solution will be
A) acidic.
B) basic
C) neutral.
D) It is impossible to tell from the information given.
Q:
Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide._____ Ca(OH)2(aq) + _____ H3PO4(aq) -> _____ Ca3(PO4)2(aq) + _____ H2O(l)A) 3.04 mLB) 15.0 mLC) 22.5 mLD) 33.8 mL
Q:
In an acid-base neutralization reaction 38.74 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. 194 M
B) 0. 387 M
C) 0. 775 M
D) 1.29 M
Q:
How many milliliters of 0.550 M hydriodic acid are needed to react with 15.00 mL of 0.217 M CsOH?HI(aq) + CsOH(aq) -> CsI(aq) + H2O(l)A) 0. 0263 mLB) 0.169 mLC) 5.92 mLD) 38.0 mL
Q:
If 100. mL of 0.400 M Na2SO4 is added to 200. mL of 0.600 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.
A) 0.534 M
B) 0.667 M
C) 1.00 M
D) 1.40 M
Q:
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce1.38 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) 25.5 mLB) 43.1 mLC) 51.1 mLD) 102 mL
Q:
When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed?AgNO3(aq) + NH4Cl(aq) -> AgCl(s) + NH4NO3(aq)A) 1.07 gB) 2.24 gC) 3.31 gD) 6.44 g
Q:
How many grams of CaCl2 are formed when 15.00 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(s) + 2 H2O(l)A) 0.00 197 gB) 0.00 394 gC) 0.0 0789 gD) 0.0 507 g
Q:
How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3?Na2S(aq) + 2 AgNO3(aq) -> 2 NaNO3(aq) + Ag2S(s)A) 24.2 mLB) 48.5 mLC) 66.0 mLD) 96.9 mL
Q:
A student prepared a stock solution by dissolving 10.0 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 water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?
A) 0. 274 M
B) 0. 356 M
C) 2.81 M
D) 3.65 M
Q:
A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution.
He took 4.00 mL of the stock solution and 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) 0.0 197 g
B) 0.0 394 g
C) 0.0 542 g
D) 0. 108 g
Q:
A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make
450. mL of a solution that is 0.300 M in Cl- ion?
A) 0.771 mL
B) 257 mL
C) 771 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. 35 L of a 3.5 M solution?
A) 0. 14 mL
B) 0.90 mL
C) 140 mL
D) 900 mL
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) 7.32 LB) 11.1 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 these 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, C O2, 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) 0.00 829 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 dichlorodifluoro methane, C Cl2F2?
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 fluorine gas?
A) 19.0 g/mol
B) 38.0 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:
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 M
B) 0.250 M
C) 0.375 M
D) 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:
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 product
B) 1.0 mol product
C) 2.0 mol product
D) 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 write 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.
Q:
The following diagrams represent the reaction of A2 (shaded spheres) with B2 (unshaded spheres). Identify the limiting reactant and write 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