At a fixed temperature, equal moles of H2 (g) and O2 (g) are mixed in a constant pressure container (the volume of the container changes in order to keep the pressure at aconstant value). The H2 (g) and 02 (g) are allowed to react, producing H20 (g):2 H2 (9) + 02 (g) - 2 H20 (g)If the initial volume of the container, before any reaction takes place, is 4.20 L, determine the volume of the container after the H2 (g) and Oz (g) have reacted to completion.The final volume will beSubmit Answer Tries 0/15

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At a fixed temperature, equal moles of Hz (9) and Oz (9) are mixed in a constant pressure container (the volume of the container changes in order to keep the pressure at constant value). The H2 (9) and 02 (9) are allowed to react, producing Hy0 (9): 2 H2 (0) + Oz (9) – 2 H,0 (9) If the initial volume of the container, before any reaction takes place, is 4.20 L, determine the volume of the container after the H2 (9) and Oz (9) have reacted to completion. The final volume will be C

At a fixed temperature, equal moles of Hz (9) and Oz (9) are mixed in a constant pressure container (the volume of the container changes in order to keep the pressure at constant value). The H2 (9) and 02 (9) are allowed to react, producing Hy0 (9): 2 H2 (0) + Oz (9) – 2 H,0 (9) If the initial volume of the container, before any reaction takes place, is 4.20 L, determine the volume of the container after the H2 (9) and Oz (9) have reacted to completion. The final volume will be C

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 31Q

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105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
What is the value of FP for a sample of gas whose temperature is -33.0 C and volume is 0.0250 L? What temperature is required to change the volume to 66.9 cm3?
84 Consider a sample of an ideal gas with n and T held constant. Which of the graphs below represents the proper relationship between P and V? How would the graph differ for a sample with a larger number of moles?
In the Mthode Champenoise, grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Fermentation of 750. mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25C? (The density of ethanol is 0.79 g/cm3.)
94 Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of the methane can be captured and the daily production of the mine is 580 metric tons of coal, how many moles of methane could be obtained per day?
5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?
A 3.00-L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0C. a How much (what fraction) of the total pressure in the flask is due to the N2? b The flask is cooled and the pressure drops. What happens, if anything, to the mole fraction of the O2 at the lower temperature? c L of liquid water is introduced into the flask containing both gases. The pressure is then measured about 45 minutes later. Would you expect the measured pressure to be higher or lower? d Given the information in this problem and the conditions in part c, would it be possible to calculate the pressure in the flask after the introduction of the water? If it is not possible with the given information, what further information would you need to accomplish this task?

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