A 1:3 mixture of CO and H2 is passed through a catalyst to produce methane at...

A 1:3 mixture of CO and H2 is passed through a catalyst to produce methane at 500 K. CO(g) + 3H2(g) = CH4(g) + H2O(g) How much heat is liberated in producing a mole of methane? How does this compare with the heat obtained from burning a mole of methane at this temperature? How does the heat of combustion of CH4 compare with the heat of compustion of CO+3H2? (Answers: 206.11 kJ is liberated; Burning CH4 liberates 802.34 kJ; Burning CO + 3H2 liberates 1008.45 kJ).

Expert Solution

The heat of combustion (ΔH⁰c) is the energy released in the form of heat when a compound undergoes complete combustion with oxygen under standard condition. Combustion is an oxidation reaction.

It is generally expressed in units of higher heating value, lower heating value and gross heating value. The calorific value of a substance (fuel or food ) is the amount of heat released during the combustion of a specified amount of that subatance.. It may be calculated as the difference between the heat of formation (ΔH⁰f) of the products and reactants.

Combustion is exothermic reaction because the double bond in molecular oxygen is much weaker than other double bonds or pairs of single bonds, specially those in carbon dioxide and water, conversion of the weak bonds in O₂ to the stronger bonds in CO₂ and H₂O releases energy as heat.

Bond energy of CO (triple bond) is 1079 KJ/mol and methane(single bond) is 414KJ/mol.

1 mole of CO = 28 g and 1 mole of CH₄ = 16 g

CO(g) + 3H₂(g) CH₄(g) + H₂O(g) Heat = 1008.45 KJ
CH₄_(g) + 2O_2(g) CO_2(g) + 2H₂O_(l) Heat = 802.34 KJ

During combustion all the covalent bonds in the reactant are broken, amount of heat liberated in the reaction is related to the strength of these bonds and the strength of the bonds formed in the products So it can provide information about the structure of molecules and differences in this heat of combustion value shows structural variations within the molecules.

queen_honey_blossom answered 2 years ago

Methane is synthesized with a stoichiometric mixture of CO and H2 that is produced via a...

Methane is synthesized with a stoichiometric mixture of CO and H2 that is produced via a large scale coal gasification process CO + 3H2 = CH4 + H2O over Ni/Alumina catalyst. (a) What is the equilbrium conversion you can get at 400oC and 1 atm? (b) Because of exothermic nature of the reaction, reaction temperature inside a large scale commercial reactor could be raised to 700oC even if the feed temperature is kept at 350oC. Estimate the equilibrium conversion at...

A mixture of toluene and air is passed through a cooler where some toluene is condensed....

A mixture of toluene and air is passed through a cooler where some toluene is condensed. One thousand cubic feet of gases enter the cooler per hour at 100 oC and 100 mm Hg gauge. The partial pressure of the toluene in this mixture is 300 mm Hg. If 720 ft3 / hr of gaseous mixture comes out of the cooler at 50 oC and barometric pressure of 760 mm Hg. Calculate the pounds of toluene removed per hour in...

A vessel contains a gaseous mixture of composition by volume 80% H2, and 20% CO.

A vessel contains a gaseous mixture of composition by volume 80% H2, and 20% CO. It is desired that the mixture should be made in the proportion 50% H2 and 50% CO by removing some of the mixture and adding some CO. Calculate, per kilomole of mixture, the mass of mixture to be removed and the mass of CO to be added. The pressure and temperature in the vessel remain constant during the process. Take the molar mass of H2...

A gaseous mixture of 25% CO, 25% CO2, 25% H2 and 25% H20 is brought to...

A gaseous mixture of 25% CO, 25% CO2, 25% H2 and 25% H20 is brought to a temperature T and 1atm. Equilbirium composition of the gas mixture is determined by the following reaction CO2 + H2 = CO + H20. Calulate the equilbirium composition of the gaseous phase at 700K and at 1500K. Given G at 700K is 14kJ and at 1500K is -9.6kJ

1.The total pressure of a mixture of O2(g) and H2(g) is 1.95 atm. The mixture is...

1.The total pressure of a mixture of O2(g) and H2(g) is 1.95 atm. The mixture is ignited and the resulting water is removed. The remaining mixture is pure H2(g) and exerts a pressure of 0.210atm when measured at the same temperature and volume as the original mixture. What were the mole fractions of O2(g) and H2(g) in the original mixture?

1. Methane and oxygen exist in a stoichiometric mixture at 500 kPa and 298 K. They...

1. Methane and oxygen exist in a stoichiometric mixture at 500 kPa and 298 K. They are ignited and react at constant volume. Combustion is complete. a. Find the heat removed from the system per kmol of fuel if the final products are at 1500 K. b. What is the final pressure? c. Explain what assumptions made in this calculation are less accurate for constant volume combustion than for the constant pressure combustion we have studied before. d. If the...

A gas stream containing 3% A is passed through a packed column to remove 99% of...

A gas stream containing 3% A is passed through a packed column to remove 99% of A by absorption in water. The absorber will operate at 25 C and 1 atm, and the gas and liquid rates are to be 20 mole/h ft2 and 100 mole/h ft2 respectively. Mass transfer coefficient and equilibrium data are as follows: y* = 3.1 x at 25 C k_xa = 60 mol/h ft3 unit mol fraction k_ya = 15 mol/h ft3 unit mol fraction...

From a combustion process using a mixture of methane (1)/ethane (2) as fuel, the ORSAT analysis...

From a combustion process using a mixture of methane (1)/ethane (2) as fuel, the ORSAT analysis of the stack gases is given in the table below: Component Xi (molar basis) CO2 0.0769 O2 0.0837 N2 0.8394 Assume that 100 kgmole of stack gases are produced. DETERMINE: 1. Sketch the process. Label all streams. 2. Write the chemical reaction(s) that take place during the process 3. Find the composition of the fuel (mole fraction) 4. Find the % excess air.

CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1360...

CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1360 torr and a H2O partial pressure of 1768 torr at 2000 K. Part A Calculate the equilibrium partial pressure of CO2 and H2 ? torr

Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...

Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1336 torr and a H2O partial pressure of 1764 torr at 2000 K. Part A Calculate the equilibrium partial pressure of CO2. Part B Calculate the equilibrium partial pressure of H2.

Question