The reform reaction between steam and gaseous methane (CH,) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 255. liters per second of methane are consumed when the reaction is run at 257. °C and the methane is supplied at 0.62 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. kg do

The reform reaction between steam and gaseous methane (CH,) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 255. liters per second of methane are consumed when the reaction is run at 257. °C and the methane is supplied at 0.62 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. kg do

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter4: Introduction To Gases

Section: Chapter Questions

Problem 67E: The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the...

See similar textbooks

Similar questions

Butane, C4H10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.857 atm and 22C. Give the answer in grams per liter
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?
Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?
A four-liter tank is filled with propane gas, C3H8. The mass of the tank filled with gas is 1236 g. The pressure in the tank is 2.68 atm. The temperature in the room is 37C. The propane in the tank is used up under the same conditions of temperature and pressure. What is the mass of the empty tank?
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.)
88 Liquid oxygen for use as a rocket fuel can be produced by cooling dry air to 183°C, where the O2 condenses. How many liters of dry air at 25°C and 750 torr would need to be processed to produce 150 L of liquid O2 at 183°C? (The mole fraction of oxygen in dry air is 0.21, and the density of liquid oxygen is 1.14g/mL.)
What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 C and 74-4 torr?
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
60 Automakers are always investigating reactions for the generation of gas to inflate air bags, in part the because the sodium produced in the decomposition of NaN3 (see Problem 5.59) presents safety concerns. One system that has been considering is the oxidation of graphite by Strontium nitrate, as Sr(NO3)2as shown in the equation below: 5C(s)+2Sr(NO3)2(s)2SrO(s)+2N2(g)+5CO2(g) . Suppose that a System is being designed using this reaction and the goal is to generate enough gas to inflate a bag 61 L and 1.3 atm at 23 C. What is the minimum mass of graphite that should be used in the design of this system?
A 275-mL sample of CO gas is collected over water at 31C and 755 mmHg. If the temperature of the gas collection apparatus rises to 39C, what is the new volume of the sample? Assume that the barometric pressure does not change.
The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the compression stroke to the pressure in the beginning. Assume that compression occurs at constant temperature. The total volume of the cylinder in an automobile is 350 cm3, and the displacement the reduction in volume during the compression stroke is 309 cm3. What is the compression ratio in that engine?
An intermediate reaction used in the production of nitrogen-containing fertilizers is that between ammonia and oxygen: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) A 150.0-L reaction chamber is charged with reactants to the following partial pressures at 500C: PNH3=1.3atm, PO2=1.5atm. What is the limiting reactant?