Part A Calculate the density of oxygen, O2, under each of the following conditions: • STP • 1.00 atm and 30.0 °C Express your answers numerically in grams per liter. Enter the density a STP first and separate your answers by a comma. • View Available Hint(s) ΑΣΦ density at STP, density at 1 atm and g/L 30.0 °C = Submit Part B To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 1.5-L bulb, then filled it with the gas at 2.00 atm and 21.0 °C and weighed it again. The difference in mass was 3.5 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ

Part A Calculate the density of oxygen, O2, under each of the following conditions: • STP • 1.00 atm and 30.0 °C Express your answers numerically in grams per liter. Enter the density a STP first and separate your answers by a comma. • View Available Hint(s) ΑΣΦ density at STP, density at 1 atm and g/L 30.0 °C = Submit Part B To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 1.5-L bulb, then filled it with the gas at 2.00 atm and 21.0 °C and weighed it again. The difference in mass was 3.5 g. Identify the gas. Express your answer as a chemical formula. • View Available Hint(s) ΑΣφ

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 74E: Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially...

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The density of air at 20C and 1.00 atm is 1.205 g/L. If this air were compressed at the same temperature to equal the pressure at 50.0 m below sea level, what would be its density? Assume the barometric pressure is constant at 1.00 atm. The density of seawater is 1.025 g/cm3.
Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
A 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?
Given 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?
97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
In the discussion on the composition of air, mention is made of the fact that water vapor may have a concentration as high as 40,000 ppm. Calculate the partial pressure exerted by water vapor at this concentration. Assume that this represents a situation with 100% humidity. What temperature would be needed to achieve this value? (See Appendix G.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
One 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.
Calculate the density of Oxygen under the condition of -STP -1.00atm and 25.0 degrees Celcius.
Nickel carbonyl, Ni(CO)4, is one of the most toxic substancesknown. The present maximum allowable concentrationin laboratory air during an 8-hr workday is 1 ppb(parts per billion) by volume, which means that there isone mole of Ni(CO)4 for every 109 moles of gas. Assume24 °C and 1.00 atm pressure. What mass of Ni(CO)4 is allowablein a laboratory room that is 12 ft x 20 ft x 9 ft?
1. What volume of water vapour (in L) will be produced during the production 291 L of hydrogen cyanide?Assume all reactant and product volumes are measured at 300 kPa and 1200 oC. 2. What volume (in L) does a 3.88 mol sample of hydrogen gas occupy at STP?(Do not show your work in the space provided; record only your final answer with the correct number of significant digits and the proper units.) 3. What volume (in L) does a 1.27 g sample of chlorine gas occupy at SATP? 4. What mass of helium gas (in g) occupies 12.4 L at STP? 5. What is the mass (in g) of a 32.9 L sample of carbon dioxide gas at a temperature of 30.0 oC and a pressure of 113 kPa?