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Concept explainers
(a)
Interpretation:
Volume occupied by
Concept Introduction:
Real gases consist of atoms or molecules that have intermolecular attractions as well as repulsions. These gases deviate from ideal gases in terms of intermolecular forces. Such gases obey van der Waals equation. Van der Waals equation is as follows:
Here,
Significance of attractive forces is determined by factor
(a)
Interpretation:
Volume occupied by
Concept Introduction:
Refer to part (a).
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Chapter 3 Solutions
Chemical Principles: The Quest for Insight
- A 0.495 g sample of a metal, M, reacts completely with sulfuric acid according to M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 225 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass= ? g/molarrow_forwardA 0.244 g sample of a metal, M, reacts completely with sulfuric acid according to M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 255 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal.arrow_forward.53 In the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100 °C in a boiling-water bath and determine the mass of vapor required to fill the bulb. From the following data, calculate the molar mass of the unknown liquid: mass of unknown vapor, 1.012 g; volume of bulb, 354 cm; pressure, 742 torr; temperature, 99 °C. 3.arrow_forward
- A quantity of N2(g) gas occupies a volume of 1.0 L at 300 K and 1.0 atm. The gas expands to a volume of 3.0 L as the result of a change in both temperature and pressure. Find the density of the gas (in g·L–1) under these new conditions.arrow_forwardA sample of hydrogen is collected by displacing a sample of water with a temperature of 35C. The mixture has a total pressure of 114 kPa. What is the partial pressure of the dry hydrogen in kPa?arrow_forwardA 0.564 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H, (g) → A volume of 219 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol * TOOLS x10"arrow_forward
- If 0.10 mol l2 vapor can effuse from an opening in a heated vessel in 42.0 seconds, how long will it take 0.10 mol H2 to effuse under the same conditions?arrow_forwardGases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) + 2 HCI(aq) MgCla(aq) + Ha(g) The total pressure of gas collected over water is 725.0 mmHg and the temperature is 25.5°C What is the pressure of hydrogen gas formed in mmHg? Pressure = mmHgarrow_forwardThe vapor pressure of liquid mercury at 27°C is 2.87 ×10-6 atm. Calculate the number of Hg atoms per cubic centimeter in the “empty” space above the top of the column of mercury in a barometer at 27°C.arrow_forward
- In the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100 °C in a boiling-water bath and determine the mass of vapor required to fill the bulb (see drawing (Figure 1)). Part A unknown vapor, 1.013 g ; volume of bulb, 355 cm3 ; From the following data, calculate the molar mass of the unknown liquid: mass pressure, 742 torr ; temperature, 99 °C ΑΣφ. ? MM = g/mol Submit Request Answerarrow_forwardCalculate the pressure exerted by 2.56 moles of CO2 confined in a volume of 4.09 L at 459 K. What pressure is predicted by the ideal gas equation? The van der Waals constants for CO2 are a = 3.59 atm · L2/mol2 and b = 0.0427 L/mol.arrow_forwardA J-shaped tube is filled with air at 760 Torr and 22 °C. The long arm is closed off at the top and is 100.0 cm long; the short arm is 40.00 cm high. Mercury is poured through a funnel into the open end. When the mercury spills over the top of the short arm, what is the pressure on the trapped air? Let h be the length of mercury in the long arm. - Please draw a sketch to clarify the solution.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
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