Question

One method for the manufacture of “synthetic gas” is the catalytic reforming of methane with steam...

One method for the manufacture of “synthetic gas” is the catalytic reforming of methane with steam at high temperature and atmospheric pressure: CH4 (g)+ H2O(g)→ CO(g)+ 3H2 (g) The only other reaction to be considered is the water-gas-shift reaction: CO (g)+ H2O(g)→ CO2 (g)+ H2 (g) If the reactants (methane and steam) are supplied in the ratio 2 mol steam to 1 mol methane, and if heat is supplied to the reactor so that the products reach a temperature of 1,300 K, the methane is completely converted and the product stream contains 17.4 mol% CO. Assuming the reactants to be preheated to 600 K, calculate the heat requirement for the reactor.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Synthesis gas may be produce by the catalyst reforming of methane with steam. The reactions are:...
Synthesis gas may be produce by the catalyst reforming of methane with steam. The reactions are: CH4 + H2O → CO + 3H2 CO + H2O → CO2 + H2 A small plant is being to produce 1000 mol/s of hydrogen (H2) by the reactions. 280 mol/s of Methane with 100 % of excess steam (excess % relative to the reaction one) are fed to the heat exchanger at 150 °C and heated with superheated vapor. The superheated vapor inlet...
The steam reforming reaction can be described by the following two reactions: CH4 +H2O ↔ CO+3H2...
The steam reforming reaction can be described by the following two reactions: CH4 +H2O ↔ CO+3H2 CH4 +2H2O ↔ CO2 +4H2 Assume that both these reactions achieve equilibrium at 600 K. The equilibrium constants at this temperature for the two reactions are 0.41 and 1.09 respectively. Calculate the equilibrium composition if the starting composition is 5 moles of steam and 1 mole of methane at a pressure of 2 atm.
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the...
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the reaction is: CH4(g) + 2 O2(g)------>CO2(g) + 2 H2O(g)      (a) Using the following data, calculate ^H° for this reaction. ^H°f kJ mol-1:   CH4(g) = -74.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ^H° = _____ kJ (b) Calculate the total heat capacity of 1 mol of CO2(g) and 2 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...
An isobaric reactor is fed an equimolar mixture of carbon monoxide (CO) and steam (H2O) at...
An isobaric reactor is fed an equimolar mixture of carbon monoxide (CO) and steam (H2O) at 400 K and 1 bar. If 60% of the H2O is converted to H2 through the following reaction, calculate how much heat must be added to the reactor in kJ/mol H2 produced if the product stream leaves the reactor at 700 K. Assume ideal gas behavior for all species. CO(g) + H2O(g) → CO2(g) + H2(g)
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
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, 26.5 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 torr and a temperature of 125 ∘C). The reaction produces 26.0 L of hydrogen gas measured at STP. What is the percent...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
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, 26.5 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 ∘C). The reaction produces 26.2 L of hydrogen gas measured at STP. What is the percent...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g...
The most important commercial process for generating hydrogen gas is the water-gas shift reaction: CH4(g) +...
The most important commercial process for generating hydrogen gas is the water-gas shift reaction: CH4(g) + H2O(g) → CO(g) + 3H2(g) Use tabulated thermodynamic data to find ΔG° for this reaction at the standard temperature of 25°C. 1.423×102 kJ Calculate ΔG°1000 for this process when it occurs at 1000 K .
Ethylene oxides is produced by the catalytic oxidation of ethylene: C2H4 (g)+ (1/2)O2---> C2H4O (g) An...
Ethylene oxides is produced by the catalytic oxidation of ethylene: C2H4 (g)+ (1/2)O2---> C2H4O (g) An undesired competing reaction is the combustion of ethylene to CO2. The feed to a reactor contains 2 mol C2H4/mol O2. The conversion and yield in the reactor are respectively 25% and 0.70 mol C2H4O produced/mol C2H4 consumed. A multiple-unit process separates the reactor outlet stream component: C2H4 and O2 are recycled to the reactor, C2H4O is sold, and CO2 and H2O are discarded. The...
Methane gas is burned completely with 30% excess air in a furnace operating at one atmosphere....
Methane gas is burned completely with 30% excess air in a furnace operating at one atmosphere. Both the methane and air enter the furnace at 40ºC saturated with water vapor. The flue gas (furnace exhaust) leaves the furnace at 1000ºC. The flue gas then passes through a heat exchanger and emerges at 60ºC. If 260 mole/sec of methane fed to the furnace, how much heat is lost from the furnace, and how much heat is transferred in the heat exchanger?...