PRINCIPLES OF MODERN CHEMISTRY-OWLV2
8th Edition
ISBN: 9781305271609
Author: OXTOBY
Publisher: CENGAGE L
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.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.
A 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?
oxygen gas from the decomposition of KClO3 was collected by water displacement. the barometric pressure during the experiment was 723,9mmHg and the temperature was 20.0C. what is the partial pressure of oxygen collected (the vapor pressure of water at 20C is 17.5mmHg)?
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- Why is nitrogen a good choice for the study of ideal gas behavior around room temperature?arrow_forwardOne of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it gave an oxide with the formula Be2O3. This resulted in a calculated atomic mass of 13.5 for beryllium. In formulating his periodic table, Mendeleev proposed that beryllium was divalent (forming Be2+ ions) and that it gave an oxide with the formula Be2O3. This assumption gives an atomic mass of 9.0. In 1894, A. Combes (Comptes Rendus 1894, p. 1221) reacted beryllium with the anion C5H7O2and measured the density of the gaseous product. Combess data for two different experiments are as follows: I II Mass 0.2022 g 0.2224 g Volume 22.6 cm3 26.0 cm3 Temperature 13C 17C Pressure 765.2 mm Hg 764.6 mm If beryllium is a divalent metal, the molecular formula of the product will be Be(C5H7O2)2; if it is trivalent, the formula will be Be(C5H7O2)3. Show how Combess data help to confirm that beryllium is a divalent metal.arrow_forwardA breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at a barometric pressure of 101.4 kPa, if PHe = 82.5 kPa and PCO2 = 0.4 kPa?arrow_forward
- To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 2.00 molmol of gas DD measured at 251 ∘C∘C in a 1.75-LL container assuming ideal behavior?arrow_forward2. A sample of vapor weighing 0.368 g filled a Florence flask when heated in a water bath at 95.0°C. The actual volume of the flask was 128.4 mL and the barometric pressure was 747 torr. Calculate (a) the volume of the vapor at STP and (b) the molar mass of the volatile liquid. (Use the approach applied in the Introduction and on the data sheet.)arrow_forwardA sample of hydrogen gas was found to have a pressure of 125 kPa when the temperature was 23 °C. What can its pressure be expected to be when the temperature is 11 °C?arrow_forward
- Gay-Lussac’s Law The temperature of a sample of gas in a steel tank at 30.0 kPa is increasedfrom –100.0 ̊ to 1.00 x 103 ̊C to 25.0 ̊. What is the final pressure inside the tank?arrow_forward1.) Clouds of hydrogen molecules have been detected deep in an interstellar space. It is estimated that these clouds contain about 1 x 1010 hydrogen molecules per m3, and have a temperature of just 25 K. Using these data, find the approximate pressure in such a cloud. 2.) A vessel of volume 22.4 L contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.arrow_forwardA sample of oxygen gas was collected via water displacement. Because the oxygen was collected via water displacement, the sample is saturated with water vapor. The total pressure of the mixture at 26.4 °C is 1.059 bar . Calculate the partial pressure of oxygen. The vapor pressure of water at 26.4 °C is 25.81 mm Hg. Ро, bararrow_forward
- 11) The temperature of a 9382 mL sample of Ne is changed, causing a change in pressure from 121.94 kPa to 175.82 kPa. If its new temperature is 849.71K and its new volume is 310.1 mL, what was the initial temperature in Kelvin? 12) A sample of O; at -38.62 °C experiences a change in volume from 3846.8 mL to 5820.5 mL. If its new pressure is 73634.12 torr at -164.3°C, what was the initial pressure in torr?arrow_forwardYou collect a sample of hydrogen gas in an inverted buret by displacement of water at 22.0 °C. The buret could not be submerged deep enough in the water bath to equilize pressure. The water level in the buret was 14.43 cm above the water level in the water bath. The volume of gas in the buret was determined to be 32.60 mL. If the current atmospheric pressure was 29.45" of Hg, what is the pressure (torr) of dry hydrogen in the buret? How many moles of hydrogen are in this sample?arrow_forwardA sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.arrow_forward
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