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Ynthesis gas, a mixture that includes the fuels carbon monoxide and molecular hydrogen, is used p...
The H2/CO ratio in mixtures of carbon monoxide and hydrogen (called synthesis gas) is increased by the water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g), which has an equilibrium constant Kc=4.24 at 800 K. Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H2O at 800 K if only CO and H2O are present initially at concentrations of 0.132 M .
23. The reaction of carbon and water to produce "water gas", a mixture of carbon monoxide and hydrogen, is an important industrial reaction. If AH - +131.3 kJ and AS - +0.1336 kJ/K for C(s) + H20 (g) =CO(g) + H2(g), determine the temperatures at which this reaction is spontaneous under standard conditions. a. T> 1.02 x 10-K b. T< 298 K c. T< 983 K d. T < 710 K e.T> 983 K
Problem 2 (2 marks): The water gas shift reaction uses carbon monoxide to convert steam to H2. CO2 + H2 CO +H2O > This is an equilibrium reaction where the concentrations at equilibrium are determined by the equation: CCO,CH2 ССОсње 9000 a) What is the heat of reaction per mole of H2 produced? b) How much heat is produced at equilibrium if 1 mol of steam is combined with 1 mol of CO at the start? Problem 2 (2 marks):...
26. Synthesis of Hydrogen (Step 2) When the CO produced in the steam-methane reforming reaction is reacted with more steam at 450 K, the water-gas shift reaction: CO(g) + H20(g) CO(g) + H2(g) produces more hydrogen. If the equilibrium partial pressures of the gases in the reactor are 0.35 atm H2O 0.24 atm CO, 4.47 atm H2, and 4.36 atm CO2, what is the value of K?
Hydrogen and carbon dioxide can be used to produce carbon monoxide according to the water-gas shift reaction given by: H2 + CO2 = CO + H2O. If a reaction is set-up initially with n moles each of H2 and CO2 and none of either of the products, CO and H2O, and the variable x represents the fraction of H2 dissociated at equilibrium. Complete the following table in terms of n and x. H2 CO2 CO H2O Total moles Moles at...
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...
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?
The H2/COH2/CO ratio in mixtures of carbon monoxide and hydrogen (called synthesis gas) is increased by the water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g)CO(g)+H2O(g)⇌CO2(g)+H2(g), which has an equilibrium constant Kc=4.24Kc=4.24 at 800 KK. Part A Calculate the equilibrium concentrations of CO2CO2, H2H2, COCO, and H2OH2O at 800 KK if only COCO and H2OH2O are present initially at concentrations of 0.169 MM . Express your answers using three decimal places separated by commas.
The H2/CO ratio in mixtures of carbon monoxide and hydrogen (called synthesis gas) is increased by the water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g), which has an equilibrium constant Kc=4.24 at 800 K. Part A Calculate the equilibrium concentrations of CO2, H2, CO, and H2O at 800 K if only CO and H2O are present initially at concentrations of 0.129 M . Express your answers using three decimal places separated by commas. Hi I don't know how to solve this problem. Please explain...
Example At elevated temperatures, methane (CHA) reacts with water to produce hydrogen and carbon monoxide in what is known as a steam-reforming reaction: CH4(9)+H2O(g)= CO(g)+3H2(g) K= 2.4 x 10-4 at 900 K. Huge amounts of hydrogen are produced from natural gas in this way and are then used for the industrial synthesis of ammonia. If 1.2 x 10-2 mol of CH4, 8.0 x 10-3 mol of H20, 1.6 x 10-2 mol of CO, and 6.0 × 10-3 mol of H2...