Time Left: 01:59:53Xenon hexafluoride was one of the first noble gas compounds synthesized. The solid reacts rapidlywith the silicon dioxide in glass or quartz containers to form liquid XeOF, and gaseous silicontetrafluoride. What is the pressure in a 1.00 - L container at 25 deg C after 4.09 g of xenonhexafluoride reacts? (Assume that silicon tetrafluoride is the only gas present and that it occupies theentire volume.) Round your answer to 3 significant figures.Note: Reference the Fundamentalconstants table for additional information.

Answered: Time Left: 01:59:53 Xenon hexafluoride…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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13. -j When a certain acid and a certain base are mixed together, a reaction occurs that produces a gas as one of the products. The gas has a density of 1.83 g/L at 1.00 atm and 20°C. What are the molar mass and identity of the gas? a) CO, 28 g/mol b) O2, 32 g/mol c) SO2, 64 g/mol d) CO2, 44 g/mol
You wish to follow the evolution of the following conversion: N2O4(g) --> 2 NO2(g) Suppose that you start with 758 mmHg N2O4 in a closed container. When the total pressure is 1,039 mmHg, what is the pressure of N2O4? by following the changes in pressure of the gas mixture as the reaction proceed. The total pressure you measure is the sum of the pressures of N2O4 and NO2 present.
Some fire extinguishers spray gas pressure generated by the reaction of baking soda with sulfuric acid: NaHCO3(aq)+H2SO4(aq)-->CO2(g)+NaHSO4(aq)+H2O(l). Predict the pressure (atm) that could build up in a 25.0L tank if 1750.0g NaHCO3 reacted with excess H2SO4 at 35 degrees
Xenon hexafluoride was one of the first noble gas compounds synthesized. The solid reacts rapidly with the silicon dioxide in glass or quartz containers to form liquid XeOF and gaseous silicon tetrafluoride. What is the pressure in a 1.00-L container at 25 °C after 8.90 g of xenon hexafluoride reacts? (Assume that silicon tetrafluoride is the only gas present and that it occupies the entire volume.) Be sure your answer has the correct number of significant figures. 4 Note: Reference the Fundamental constants table for additional information. atm ☐ x10 X
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1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg. (R = 0.0821 atm.L/mol.K) 2) Given the following reaction of Ca(s) in HCl(aq): Ca(s) + 2 HCl(aq) --> CaCl2(aq) + H2(g) If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced. 3) An unknown gas with a mass of 1.211g occupies a volume of 677 mL. The temperature is 230C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.
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4 You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It reacts in the following: 2Ga(s)+6HCl(aq)→2GaCl3(aq)+3H2(g) You collect 171 mLs and 0.996 atm of hydrogen over water. How many moles of Ga reacted? The partial pressure of water at 28 degrees is 0.0372 atm. Rember sig figs
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A container of N,0,(g) has a pressure of 0.445 atm. When the absolute temperature of the N,O,(g) is tripled, the gas completely decomposes, producing NO, (g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change. final pressure: atm
5.72 A sample of zinc metal reacts completely with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) The hydrogen gas produced is collected over water at 25.0°C using an arrangement similar to that shown in Figure 5.15. The volume of the gas is 7.80 L, and the pressure is 0.980 atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at 25°C = 23.8 mmHg.)
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