According to the following combustion reaction, pure methanol liquid undergoes complete combustion with excess oxygen. If 55.79 liters, L of pure carbon dioxide, CO2 (water removed) was recovered at STP, how many milliliters, mL of methanol, CH3OH must have reacted? The density of liquid methanol is 0.792 g/mL. Just give the numerical value. The assumption is the answer is in milliliters, mL. Reaction: 2 CH3OH(I) + 3 O₂(g) --> 4 H₂O(g) + 2 CO₂(g)

According to the following combustion reaction, pure methanol liquid undergoes complete combustion with excess oxygen. If 55.79 liters, L of pure carbon dioxide, CO2 (water removed) was recovered at STP, how many milliliters, mL of methanol, CH3OH must have reacted? The density of liquid methanol is 0.792 g/mL. Just give the numerical value. The assumption is the answer is in milliliters, mL. Reaction: 2 CH3OH(I) + 3 O₂(g) --> 4 H₂O(g) + 2 CO₂(g)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....

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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.
Acid rain results from the reaction of nitrogen dioxide, a major component of photochemical smog which is the brown gas hanging over major cities, in the air mixing with water vapor to form nitric acid in the reaction shown below. 3NO2(g) + H2O(g) ----> 2HNO3(aq) + NO(g) Assuming this reaction is happening in the open air, when 69L of Nitrogen dioxide are reacted with water, how many liters of nitrogen monoxide will be produced in the atmosphere?
used in the manufacture of cement: ate rock (limestone) is heated to produce the quicklime, i.e., calcium oxide, Carbon dioxide is also released into the atmosphere when calcium carbon- PROBLEM 44 CACO3(s) CaO(s) + CO;(g) Calculate the mass, in metric tons, of CO2 released per metric ton of lime- une used in this process. What is the mass of carbon that the air gains for each of carbon dioxide that enters the atmosphere? Note that at least gram os much carbon dioxide is released from combustion of the fossil fuel needed to heat the limestone as is released from the limestone itself.
✓ 个 < app.101edu.co STARTING AMOUNT X How many grams of oxygen gas are produced when 2.43 x 104 g of KCIO, are completely reacted according to the following chemical equation: 3.5 1 ADD FACTOR * ( ) 32.00 9.52 x 10-5 g KCIO3 2 KCIO3(s) → 1.90 x 10-4 Question 31 of 38 2 mol KCIO3 O 3 2 KCI(S) + 3 M 74.55 mol KCI ANSWER 31 1.98 x 10-6 5.95 x 10-6 mol O₂ O₂(g) 2.43 x 104 6.022 x 10²3 g 0₂ by RESET 2 2.97 x 10-6 122.55 g KCI Feb 23 7:11 O
Hydrazine (N2H4) and hyfrogen peroxide (H2O2) have been used as rockets propellants. They react according to the following equiation. 7H2O2 + N2H4 --> 2HNO3 + 8H2O a) When 76 kg of hydrazine react, hoe many grams of nitric acid can be formed? b)When 289 mL of hydrogen peroxide (d= 1.41 g/mL) recat, how many grams of water can be formed? c)how many grams of hydrinaze will be required to react with 765 g of hydrogen peroxide? d)How many grams of water can be produced when 204 g hydrazine combined with 175 g hydrogen peroxide? e) How many of the exceess reactant in part (d) are left unreacted?
Calculate the theoretical yield in moles NH3 from the complete reaction
Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21
Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g) + (1/2)O2(g) <--> COCl2(g) + Cl2(g), Kc = 4.4 x 109 at 1,000 KCalculate Kc for the reaction 2CCl4(g) + O2(g) <--> 2COCl2(g) + 2Cl2(g). (2 sig figs)
Consider the following reactions:CoO (s) + CO (g) D CO2 (g) + Co (s) Kc(1) = 490.2 CoO (s) + 2 H2 (g) D 2 Co (s) + 2 H2O (g) Kc(2) = 4.5 x 103a. Write the overall equation for the reaction of hydrogen gas and carbon dioxide gas to produce carbon monoxide gas and steam.
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. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. x10 2. Suppose 75.0 mL of dioxygen gas are produced by this reaction, at a temperature of 80.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
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. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 0 2. Suppose 62.0 mL of dioxygen gas are produced by this reaction, at temperature of 130.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits. g 010 X 0x12
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. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. x10 2. Suppose 28.0 mL of dioxygen gas are produced by this reaction, at a temperature of 60.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits.

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