Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 1, Problem 1.69E
Using the barometric formula, calculate the expected air pressure in Colorado Springs, Colorado, which is 1840 meters above sea level. Assume a temperature of 26.0 °C.
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b)
A car tire is filled with air to 33 psi at 295 K.
i)
After a drive, the temperature inside of the tire rises to 318 K due to friction with the
road surface. If the tire volume is constant, what is the pressure (in psi)?
If the tire leaks 1.0 g of air per minute and the temperature is constant, how many
minutes will it take for the tire to reach the original pressure of 33 psi (molecular mass
of air= 28.8 g/mol).
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A sample of hydrogen gas is produced in a chemical reaction at 21.0 °C, where the hydrogen
bubbles through water before being collected. Measured from the barometer, the
atmospheric pressure of the wet gas in this experiment is 750.1 mmHg. Calculate the
partial pressure (in mmHg) of the dry hydrogen gas (no water vapor). Show all work, and
circle your final answer.
Chapter 1 Solutions
Physical Chemistry
Ch. 1 - A bomb calorimeter is a study metal vessel in...Ch. 1 - Difference between the system and the...Ch. 1 - Prob. 1.3ECh. 1 - Prob. 1.4ECh. 1 - Prob. 1.5ECh. 1 - Prob. 1.6ECh. 1 - Prob. 1.7ECh. 1 - A pot of cold water is heated on a stove, and when...Ch. 1 - hat difference is necessary for heat to flow...Ch. 1 - What is the value of FT for a sample of gas whose...
Ch. 1 - What is the value of FP for a sample of gas whose...Ch. 1 - Prob. 1.12ECh. 1 - Hydrogen gas is used in weather balloon because it...Ch. 1 - Prob. 1.14ECh. 1 - A 2.0 L soda bottle is pressurized with 4.5 atm of...Ch. 1 - The Mount Pinatubo volcano eruption in 1991...Ch. 1 - Prob. 1.17ECh. 1 - Scottish physicist W. J. M. Rankine proposed an...Ch. 1 - Use the two appropriate values of R to determine a...Ch. 1 - Prob. 1.20ECh. 1 - Pressures of gases in mixtures are referred to as...Ch. 1 - Earths atmosphere is approximately 80 N2 and 20...Ch. 1 - The atmospheric surface pressure on Venus is 90...Ch. 1 - Prob. 1.24ECh. 1 - Prob. 1.25ECh. 1 - In the anaerobic oxidation of glucose by yeast,...Ch. 1 - What are the slopes of the following lines at the...Ch. 1 - For the following function, evaluate the...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Prob. 1.31ECh. 1 - Prob. 1.32ECh. 1 - Prob. 1.33ECh. 1 - Prob. 1.34ECh. 1 - What properties of a nonideal gas do the Vander...Ch. 1 - Prob. 1.36ECh. 1 - Prob. 1.37ECh. 1 - Calculate the Boyle temperatures for carbon...Ch. 1 - Prob. 1.39ECh. 1 - Prob. 1.40ECh. 1 - Table 1.4 show that the second virial coefficient...Ch. 1 - Prob. 1.42ECh. 1 - What is the van der Waals constant a for Ne in...Ch. 1 - Prob. 1.44ECh. 1 - Under what conditions would the van der Waals...Ch. 1 - By definition, the compressibility of an ideal gas...Ch. 1 - The second virial coefficient B and the third...Ch. 1 - Use the approximation 1 x-1 1 x x2 to...Ch. 1 - Why is nitrogen a good choice for the study of...Ch. 1 - Evaluate for a gas following the Redlich-Kwong...Ch. 1 - Numerically evaluate for one mole of methane...Ch. 1 - Under what conditions of volume does a van der...Ch. 1 - At high temperatures, one of the van der Waals...Ch. 1 - Under what conditions of temperature does a...Ch. 1 - The Berthelot equation of state for one mole of...Ch. 1 - Prob. 1.56ECh. 1 - Referring to exercises 1.6 and 1.7, does it matter...Ch. 1 - Prob. 1.58ECh. 1 - Use Figure 1.11 to construct the cyclic rule...Ch. 1 - Prob. 1.60ECh. 1 - Prob. 1.61ECh. 1 - Calculate for one mole of an ideal gas at STP and...Ch. 1 - Prob. 1.63ECh. 1 - Show that = T/p for an ideal gas.Ch. 1 - Determine an expression for V/T p, n in terms of ...Ch. 1 - Prob. 1.66ECh. 1 - Prob. 1.67ECh. 1 - Perform a units analysis on the exponent of the...Ch. 1 - Using the barometric formula, calculate the...Ch. 1 - The barometric formula can also be used for...Ch. 1 - Prob. 1.71ECh. 1 - Prob. 1.72ECh. 1 - Prob. 1.73ECh. 1 - Prob. 1.74ECh. 1 - Prob. 1.75ECh. 1 - Prob. 1.76ECh. 1 - Prob. 1.77ECh. 1 - Prob. 1.78ECh. 1 - Prob. 1.79ECh. 1 - Use the ideal gas law to symbolically prove the...Ch. 1 - Prob. 1.81E
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- Oxygen Consumption If 5.00 L of hydrogen gas,measured at a temperature of 20.0°C and a pressure of80.1 kPa, is burned in excess oxygen to form water, whatmass of oxygen will be consumed? Assume temperatureand pressure remain constant.arrow_forwardGiven that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardA sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?arrow_forward
- Why is nitrogen a good choice for the study of ideal gas behavior around room temperature?arrow_forwardArgon gas exerts 1.06 atm pressure at 290 K. Determine its density in g/L.arrow_forwardIn an air-conditioned room at 21.0 ∘C, a spherical bubble had the diameter of 60.0 cm. When taken outside on a hot summer day, the bubble expanded to 61.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the bubble is a perfect sphere and that the pressure and number of moles of air molecules remains the same.arrow_forward
- A hot-air balloon will rise when the density of its air is 10.1% lower than that of the atmospheric air. Calculate the density of air at 319.7, 0.9atm (assume that dry air is 78% N2 and 22% O2) and determine the minimum temperature of air that will cause a balloon to rise.arrow_forwardThe barometric pressure measured outside an airplane was 245 mmHg. Calcuate this pressure in kPa.arrow_forwardUse the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of neon at a pressure of 500.0 atm and a temperature of 355.0 K. Explain why the two values are different. (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V.)arrow_forward
- A student reads a barometer in the laboratory and finds the atmospheric pressure to be 793.6 mmHg. Express this pressure in atmospheres (do not include the units). Assume that the conversion is exact.arrow_forwardExperiments carried out by French chemists Jacques Alexandre César Charles and Joseph-Louis Gay-Lussac and British physicist Lord Kelvin determined a quantitative relationship between the volume and temperature of a gas. Their data showed that for a container of gas held at constant pressure, the volume and temperature are directly proportional. For example, if you inflate a balloon outdoors with cold air on a cold day and then take it inside, it will expand, and it might even burst. This happens because as the temperature of the air inside the balloon increases, the volume of the balloon increases as well. What is less obvious is the quantitative relation: If the pressure is held constant, then when the temperature is doubled, the volume is doubled as well. Part A According to Charles's law, for a fixed quantity of gas at constant pressure, which of the given quantities is constant? ► View Available Hint(s) OF O VXT O V +T Submit Part B A balloon was filled to a volume of 2.50 L when…arrow_forwardNitrogen gas is collected over water in a measuring cylinder, the level of water being the same inside and outside the cylinder. The volume of nitrogen collected was 120 mL, the temperature was read as 21 degrees celcius, Barometric pressure was observed to be 750.1 mm Hg. A.) Calculate the mass of nitrogen if the partial pressure of water at this temperature is 18.7 mmHg. B.) Calculate the volume of dry nitrogen if the conditions were changed to obtained at 298 K and 1 atm.arrow_forward
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