J9 cmsingi eltha noitulos eucoupe M 00 ebixonbyr Oxidation-Reduction Stoichiometry PL sin (1)ego to 1. When 50.0 mL of a 0.500 M copper (II) sulfate solution is mixed with 1.56 grams of aluminum. Write the balanced equation. +2 2 Al (s) + 3 Cu²² (50₁j ²) (aq) → +3 2 Al±³ (sou³) 3 (aq) +3 Cu (s) b. What mass of copper is produced? C. How much excess reactant remains at the end of the reaction? hero erit we s(OM)=8 to uxim tubong art we 10 sen edr prie US ups 2. Throwing some scrap iron in a gold nitrate solution causes the gold metal to precipitate. What volume 0.50 M gold nitrate solution would react with 224 grams of iron metal? 3 Fe(s) + 2 Au(NO3)3(aq) 3 Fe(NO3)2(aq) + 2 Au (s) 3. How many ml of 2.50 M HNO3 contain enough nitric acid to dissolve an old copper penny with a mass of 3.94 grams? 0.002 w pr 3 Cu(s) + 8 HNO3(aq) 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H20(1) rit onial (CM) to noiule M 00 is to Jm As 4. In the oxidation of silver, if 45.0 grams of silver sulfide is produced from excess exposure to sulfur containing compounds, how much silver tarnished? YOX

J9 cmsingi eltha noitulos eucoupe M 00 ebixonbyr Oxidation-Reduction Stoichiometry PL sin (1)ego to 1. When 50.0 mL of a 0.500 M copper (II) sulfate solution is mixed with 1.56 grams of aluminum. Write the balanced equation. +2 2 Al (s) + 3 Cu²² (50₁j ²) (aq) → +3 2 Al±³ (sou³) 3 (aq) +3 Cu (s) b. What mass of copper is produced? C. How much excess reactant remains at the end of the reaction? hero erit we s(OM)=8 to uxim tubong art we 10 sen edr prie US ups 2. Throwing some scrap iron in a gold nitrate solution causes the gold metal to precipitate. What volume 0.50 M gold nitrate solution would react with 224 grams of iron metal? 3 Fe(s) + 2 Au(NO3)3(aq) 3 Fe(NO3)2(aq) + 2 Au (s) 3. How many ml of 2.50 M HNO3 contain enough nitric acid to dissolve an old copper penny with a mass of 3.94 grams? 0.002 w pr 3 Cu(s) + 8 HNO3(aq) 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H20(1) rit onial (CM) to noiule M 00 is to Jm As 4. In the oxidation of silver, if 45.0 grams of silver sulfide is produced from excess exposure to sulfur containing compounds, how much silver tarnished? YOX

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.98PAE

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Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.
4-77 To convert 1 mol of iron(III) oxide to its elements requires 196.5 kcal: How many grams of iron can be produced if 156.0 kcal of heat is absorbed by a large-enough sample of iron(III) oxide?
The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g) (a) What is the maximum mass of iron, in grams, that can be obtained from 454 g (1.00 lb) of iron(III) oxide? (b) What mass of CO is required to react with 454 g cot Fe2O3?
Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4, by the reaction 3NaOH(aq)+H3PO4(aq)Na3PO4(aq)+3H2O(l) The sodium hydroxide solution, whose density is 1.133 g/mL, contains 12.0% NaOH by mass.
One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?
4-81 (Chemical Connections 4C) Balance the lithium iodine battery redox reaction described in this sec tion and identify the oxidizing and reducing agents present.
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
What is Hrxn for reaction of iron(III) oxide and carbon monoxide to give iron metal and carbon dioxide gas? Use the following reactions: 4Fe(s)+3O2(g)2Fe2O3(s)H=1648.4kJ4CO(g)+O2(g)2CO3(g)H=565.98kJ
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.

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