A 8.00 L tank at 24.8 °C is filled with 19.2 g of boron trifluoride gas and 13.4 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. mole fraction gas boron trifluoride carbon monoxide Check Explanation Prive Terms of Use O 2019 McGraw-Hill Education. All Rights Reserved. 11 4X 12/ 99+ OType here to search hp ins prt sc delete f1o f6 backspace & $ vaing eyLevng eSEO ON ARES ON Battery IC 6499 R

A 8.00 L tank at 24.8 °C is filled with 19.2 g of boron trifluoride gas and 13.4 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. mole fraction gas boron trifluoride carbon monoxide Check Explanation Prive Terms of Use O 2019 McGraw-Hill Education. All Rights Reserved. 11 4X 12/ 99+ OType here to search hp ins prt sc delete f1o f6 backspace & $ vaing eyLevng eSEO ON ARES ON Battery IC 6499 R

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter9: Gases

Section: Chapter Questions

Problem 101E: Under which of the following sets of conditions does a real gas behave most like an ideal gas, and...

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Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?
Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressure
Describe the factors responsible for the deviation of the behavior of real gases from that of an ideal gas.
Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation: HN3O(g)N2(g)+H2(g) If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.
Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do this, calculate a value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). On a graph show the apparent molar mass versus the pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?
Explain why the plot of PV for CO2 differs from that of an ideal gas.
A mixture of cyclopropane and oxygen is sometimes used as a general anesthetic. Consider a balloon with an anesthetic mixture of cyclopropane and oxygen at 170. torr and 570. torr, respectively. Calculate the mole fraction of cyclopropane in the mixture.
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.