Syngas (CO+ H2) can be produced by reacting methane with water in the following reaction: CH4(g) + H2O(g) --> CO(g) + 3H2(g).
If you want to maximize the syngas products at equilibrium, should you:
(a) run the reaction at high or low temperature?
(b) run the reaction at high or low total pressures?
Briefly explain your answer.
Syngas (CO+ H2) can be produced by reacting methane with water in the following reaction: CH4(g)...
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O(g) = 3H2(g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.13 M; H20,0.239 M; CO, 0.136 M; H2 1.21 M, at a temperature of 760 °C?
CH4(g) + H2O(g) >>> CO(g) + 3H2(g) A 200. L reaction vessel containing methane (CH4) at 480K has a pressure of 1.81 atm. 16.2 moles of steam are introduced, and the reaction above takes place. What is the partial pressure of each of the four gases in this balanced equation after the reaction runs to completion? Assume that both volume and temperature remain constant.
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?
Methane and water react to form hydrogen and carbon monoxide, like this: CH4(9)+H2Og)H2)+CO) The reaction is endothermic. Suppose a mixture of CH, H,O, 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. change in composition shift in equilibrium O to the right O to...
22. How much energy is produced or absorbed when 7.9 g of methane, CH4(g), is produced in the following reaction? 3H2(g) + CO(g) CH4(g) + H2O(g) 20 aa OH = (- 74.6) . (- 241.3) — (- 10.5) = - 205, кт ДНІ: - 205.5 кі | AH CHy = - 74.6 kJ/mol AH HO = - 241,8 kg/mol AH co = -110.5 kJ/mol
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?
what are the products of the combustion reaction of methane CH4, with oxygen CO2(g) and H2O(g) C(s), and H2O(g) H2CO3(aq) CO2(g) only CO(g) and H2(g)
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)?CO(g)+3H2(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 ?C) is mixed with 22.6 L of water vapor (measured at a pressure of 700 torrand a temperature of 125 ?C). The reaction produces 27.0 L of hydrogen gas measured at STP. What is the percent yield...
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...
Consider the steps in coal gasification: C(coal) + H2O(g) - CO(g) + H2(g) Hºrn = 129.7 kJ CO(g) + H2O(g) - CO2(g) + H2(g) AH rxn = -41 kJ CO(g) + 3H2(g) → CH4(g) + H2O(g) AH'rxn=-206 kJ Calculate the heat of reaction, AH rxn, for overall reaction for the production of methane, CH4.