Wine goes bad soon after opening because the ethanol (CH,CH,OH) dissolved in it reacts with oxygen (0,) gas to form water and aqueous acetic acid (CH,COOH), the main ingredient in vinegar. Calculate the moles of ethanol needed to produce 2.40 mol of water. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.

Wine goes bad soon after opening because the ethanol (CH,CH,OH) dissolved in it reacts with oxygen (0,) gas to form water and aqueous acetic acid (CH,COOH), the main ingredient in vinegar. Calculate the moles of ethanol needed to produce 2.40 mol of water. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 114E: a. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and...

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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.
a. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and carbon dioxide gas. b. Assuming gasoline is 100.% isooctane, with a density of 0.692 g/mL, what is the theoretical yield of carbon dioxide produced by the combustion of 1.2 1010 gal of gasoline (the approximate annual consumption of gasoline in the United States)?
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. Suppose 48.0mL of dioxygen gas are produced by this reaction, at a temperature of 100.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
Ammonium perchlorate NH4ClO4 is a powerful solid rocket fuel, used in the Space Shuttle boosters. It decomposes into nitrogen N2 gas, chlorine Cl2 gas, oxygen O2 gas and water vapor, releasing a great deal of energy. Calculate the moles of oxygen produced by the reaction of 0.075mol of ammonium perchlorate. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O.Suppose 61. g of hydrobromic acid is mixed with 44.1 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits. I keep getting this problem wrong because of the sig. digits, dont round till the end because if it is off by 0.1, it will be incorrect.
Many home barbecues are fueled with propane gas (C3H8). What mass of carbon dioxide is produced upon the complete combustion of 14.5 L of propane.?Assume that the density of the liquid propane in the tank is 0.621g/mL(express answer in kilograms)
Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. Determine whether the data given confirm the formula of the hydrate. You must show any relevant calculation
The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.
When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A student prepares aspirin using 2.56 grams of salicylic acid (MW = 138 g/mol) and 4.85 mL of acetic anhydride (MW = 102 g/mol, density = 1.081 g/mL). How many moles of aspirin may be formed from the initial acetic anhydride used? Note: Your answer is assumed to be reduced to the highest power possible.
How would the following errors affect the empirical formula for the compound? The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know? The student recorded the mass of the cup + sample incorrectly and started with 2.2 g of hydrated compound but used 2.0 g in the calculations. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know?
How many grams of NaH2PO4 are needed to react with 79.12 ml of 0.834 M NaOH? Be sure your answer has the correct number of significant figures.
320.4 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen. The products of this reaction are liquid water and gaseous carbon dioxide. How much water (in kg) do you expect from this reaction assuming that all of the isomaltitol reacts? Enter your numeric answer in the units of kg. Do not enter the unit. Use enough significant digits to prevent rounding errors. Hint: balance the reaction first. Recall that 1 kg = 1000 g.

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