A 1.000-L vessel contains a mixture of hydrogen, carbon monoxide and methane gases in unknown proportions at 20.0-bar and 25 °C. The gaseous mixture is found to have a mass of 12.80-g and a higher heating value of 342.60 kJ/mol. What is the composition of the gas?
A 1.000-L vessel contains a mixture of hydrogen, carbon monoxide and methane gases in unknown proportions...
A 1.000-L vessel contains a mixture of hydrogen, carbon monoxide and methane gases in unknown proportions at 23.5-bar and 25 °C. The gaseous mixture is found to have a mass of 12.70-g and a higher heating value of 353.40 kJ/mol. What is the composition of the gas? y(H2) = ? y(CO) = ? y(CH4) = ?
Steam reforming of methane (CH) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many Important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 38. mol of methane gas and 37. mol of water vapor at 42.0°C. She then raises the temperature, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 26. moll Calculate the concentration...
Methane (CH4) is reacted with oxygen to form syngas, a mixture of carbon monoxide (CO) and hydrogen (H2). The reaction is conducted in a cylinder of volume 1 m3. 5.1 Write down the balanced reaction equation [1] 5.2 Initially the cylinder is filled with 30 mol of CH4 and 10 mol of O2. What is the pressure in the cylinder before reaction, assuming the gases are ideal? [1] 5.3 What is the gas composition (mol%) after the reaction, if the...
Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700.0 K is Kp=1.60×10−3. If a 1.55-L reaction vessel initially contains 174 torr of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium. Please show step by step solutions. Thank you!
An equilibrium mixture of water vapor, methane, carbon monoxide, and hydrogen at 1400 K has the composition: [H2O] = 9.0 M, [CH4] = 8.0 M, [CO] = 2.0 M, [H2] = 6.0 M, for the equilibrium, H2O(g) + CH4(g) ↔ CO(g) +3H2(g). If the initial reaction mixture was composed only of water vapor and methane gas, what was the initial concentration of the methane in molarity units?
Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700.0 KK is Kp=1.60×10−3Kp=1.60×10−3. If a 1.55-LL reaction vessel initially contains 249 torr of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.
1- A mixture of hydrogen and argon gases, in a 8.69 L flask at 77 °C, contains 0.477 grams of hydrogen and 7.10 grams of argon. The partial pressure of argon in the flask is ____ atm and the total pressure in the flask is ____ atm. 2- A mixture of methane and carbon dioxide gases is maintained in a 7.86 L flask at a pressure of 1.93 atm and a temperature of 39 °C. If the gas mixture contains...
A mixture of methane and hydrogen gases contains methane at a partial pressure of 193 mm Hg and hydrogen at a partial pressure of 461 mm Hg. What is the mole fraction of each gas in the mixture? XCH4 = XH2 =
Methane and water react to form hydrogen and carbon monoxide, like this: The reaction is endothermic. Suppose a mixture of CH4, H20, H2 and CO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right to the left...
A mixture of hydrogen and carbon dioxide gases is maintained in a 6.42 L flask at a pressure of 2.97 atm and a temperature of 28 °C. If the gas mixture contains 1.02 grams of hydrogen, the number of grams of carbon dioxide in the mixture is _____ g