A 8.00 L tank at 0.72 °C is filled with 10.9 g of boron trifluoride gas and 7.07 g of dinitrogen monoxide gas. You can assume both gases behave as ideal gasesunder these conditions.Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.mole fraction:boron trifiuoridepartial pressure:O atmmole fraction:dinitrogen monoxidepartial pressure:Total pressure in tank:I aim

Given : Mass of BF3 = 10.9 g Mass of dinitrogen monoxide = 7.07g

Answered: 8.00 L tank at 0.72 °C is filled with…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

ChapterC: Mathematics For General Chemistry

Section: Chapter Questions

Problem 2P

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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?
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.
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Consider a 5.00-L tank containing 375 g of Ar at a temperature of 25 C. (a) Calculate the pressure in the tank using both the ideal gas law and the van der Waals equation. (b) Which correction term, a(n/V)2 or bn, has the greatest influence on the pressure of this system?
Describe the factors responsible for the deviation of the behavior of real gases from that of an ideal gas.
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?
The following figure shows three 1.00-L bulbs connected by valves. Each bulb contains argon gas with amounts proportional to the number of circles pictorially represented in the chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that the valves connecting the bulbs are closed and seal the gases in their respective chambers. Assume also that the volume between each bulb is negligible. (a) Which bulb has the highest pressure? (b) If the pressure in bulb A is 0.500 atm, what is the pressure in bulb C? (c) If the pressure in bulb A is 0.500 atm, what is the total pressure? (d) If the pressure in bulb A is 0.500 arm, and the valve between bulbs A and B is opened, redraw the figure shown above to accurately represent the gas atoms in all three bulbs. What is P A+P B+P C? Compare your answer in part (d) to that in part (c). (e) Follow the instructions of part (d) but now open only the valve between bulbs B and C.

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