I Review | Constants | Periodi rail A What is the percent yield of the reaction? • View Available Hint(s) Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g) + H20(g) → CO(g) + 3H2(g) % In a particular reaction, 26.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 °C) is mixed with 22.2 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 °C). The reaction produces 26.4 L of hydrogen gas at STP. Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining

I Review | Constants | Periodi rail A What is the percent yield of the reaction? • View Available Hint(s) Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g) + H20(g) → CO(g) + 3H2(g) % In a particular reaction, 26.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 °C) is mixed with 22.2 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 °C). The reaction produces 26.4 L of hydrogen gas at STP. Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining

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

Chapter5: Gases

Section: Chapter Questions

Problem 101E: At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A...

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Methanol (CH3OH) can be produced by the following reaction: CO(g)+2H2(g)CH3OH(g) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?
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.)
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)
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?
A student reacts a sample of Alka-Seltzer (the reactive ingredient is NaHCO3)with hydrochloric acid and obtains the following data (note that the carbondioxide product that was evolved during the reaction was collected andmeasured):PCO2 = 656.7 torr VCO2 = 16.75 mL TCO2 = 27.0 CWhat was the mass (in grams) of the NaHCO3 present in the original Alka-Seltzersample? (Useful constant: R = 0.08206 Latm/molK)a) 0.0494 gb) 0.0474 gc) 0.0615 gd) 0.0923 g
In 2014, the World Anti-Doping Agency announced that Xenon gas would be added to the list of banned substances for athletes. Apparently since 2004, Russian athletes had been inhaling xenon while training, with the physiological effect being to boost the capacity of blood to carry oxygen needs for aerobically demanding sports. If an athlete inhaled an average of 1.75 x 10-4 moles of Xe per breath while sleeping, with an average rate of 13.0 breaths per minute for 8.50 hours how many total GRAMS of Xe(g) were inhaled while sleeping? please show all calculations