At moderate pressures (~ 200 atm), the measured pressure exerted by CO, gas is less than that predicted by the perfect gas equation. This is mainly becauseCO2 will condense to a liquid at 200 atm pressure.the volume occupied by the CO2 molecules themselves becomes significant.such high pressures cannot be accurately measured.gas phase collisions prevent CO, molecules from colliding with the walls of the containerof attractive intermolecular forces between CO, moleculesООООО

Answer - The correct option is (e) - of attractive intermolecular force between co2 molecule…

Answered: At moderate pressures (~ 200 atm), the…

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 89E

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99 Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2dimerizes, or combines with itself, to produce a mixture of NO2 and N2O4. A particular mixture of NO2, and N2O4 has a density of 2.39 g/L at 50°C and 745 torr. What is the partial pressure of NO2 in this mixture?
A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 tor. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)
The oxides of Group 2A metals (symbolized by M here) react with carbon dioxide according to the following reaction: MO(s)+CO2(g)MCO3(s) A 2.85-g sample containing only MgO and CuO is placed in a 3.00-L container. The container is filled with CO2 to a pressure of 740. torr at 20.C. After the reaction has gone to completion, the pressure inside the flask is 390. torr at 20.C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.
Workers at a research station in the Antarctic collected a sample of air to test for airborne pollutants. They collected the sample in a 1.00-L container at 764 torr and 20 C. Calculate the pressure in the container when it was opened for analysis in a particulate-free clean room in a laboratory in South Carolina, at a temperature of 22 C.
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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