1. The oxidation of nitrogen oxide produces nitrogen dioxide, as shown below:2NO (g) + O2 (g) → 2NO2 (g)If 0.300 moles of NO (g) and 0.100 moles of O2 (g) are reacted in a 2.50 m3 vessel at 298K, how many moles of NO2 gas will be produced? Which of the following substances has the lowest boiling point? Question 2 options: CH3Cl CF4 CHF3 CH2O CH3OH

1.here we are required to find the number of moles of product formed

Answered: 1. The oxidation of nitrogen oxide…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 54E: A person accidentally swallows a drop of liquid oxygen, O2(l), which has a density of 1.149 g/mL....

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In the Mthode Champenoise, grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Fermentation of 750. mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25C? (The density of ethanol is 0.79 g/cm3.)
Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
In a typical automobile engine, a gasoline vapor-air mixture is compressed and ignited in the cylinders of the engine. This results in a combustion reaction that produces mainly carbon dioxide and water vapor. For simplicity, assume that the fuel is C8H18 and has a density of 0.760 g/mL. (a) Calculate the partial pressures of N2 and 02 in the air before it goes into the cylinder; assume the atmospheric pressure is 734 mmHg. (b) Consider the case where the air, without any fuel added, is compressed in the cylinder to seven times atmospheric pressure, the compression ratio of many modem automobile engines. Calculate the partial pressures of N2 and O2 at this pressure. (c) Now consider the case where 0.050 mL gasoline is added to the air in the cylinder just before compression and completely vaporized. Assume that the volume of the cylinder is 485 mL and the temperature is 150C. Calculate the partial pressure of the gasoline vapor. (d) Calculate the amount (mol) of oxygen required to bum the gasoline in part (c) completely to CO2 and H2O. (e) The combustion reaction in the cylinder creates temperatures in excess of 1200K. Due to the high temperature, some of the nitrogen and oxygen in the air reacts to form nitrogen monoxide. If 10% of the nitrogen is converted to NO, calculate the mass (g) of NO produced by this combustion. (f) Hot-rod cars use another oxide of nitrogen, dinitrogen monoxide, to create an extra burst in power. When such a power boost is needed, dinitrogen monoxide gas is injected into the cylinders where it reacts with oxygen to form NO. Calculate the mass of dinitrogen monoxide that would have to be injected to form the same quantity of NO as produced in part (e). Assume that sufficient oxygen is present to do so.

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	CH₃Cl
	CF₄
	CHF₃
	CH₂O
	CH₃OH

1. The oxidation of nitrogen oxide produces nitrogen dioxide, as shown below: 2NO (g) + O2 (g) → 2NO2 (g) If 0.300 moles of NO (g) and 0.100 moles of O2 (g) are reacted in a 2.50 m3 vessel at 298K, how many moles of NO2 gas will be produced?