Please do only i) part. Please do only i) part. Question1 Combustion of methane

Question

Please do only i) part.

Please do only i) part.

Question1 Combustion of methane is via the reaction: CH, + 20,-CO, + 2H20 (1) AG 277,--788,487 (J/mole) However, CO2 and H20 will decompose by the reactions: CO2 CO +0.502 In order to calculate the final composition of the combustion products it is assumed that: Each mole of CHa first generates 1 mole of CO2 and 2 moles of H20 by reaction 1), .e. The CO2 and H20 then decompose to the simultaneous equilibria of (2) and (3) (only reactions i. Justify the assumption that each mole of CH4 reacts to form 1 mole of CO2 and 2 moles of ii. The initial composition is 1 mole CO2 and 2 moles H20 and the total pressure is 1 complete reaction. 2 and 3 are involved). H20 atmosphere. Generate a plot of the equilibrium gas composition between 1500°C and 3000°C iii Mixtures of CO-CO2-H2-H20 will involve the shift reaction: However, this reaction can be obtained by algebraic manipulation of reactions (2) and (3) so is not independent. Using the gas composition obtained in (ii) at 2500°C check whether (4) is also in equilibrium and comment on the result. R= 8.3143 (J/mole-K)

Explanation / Answer

CH4 + 2O2 = CO2 + 2H2O

From the stoichiometry of the reaction

1 mol of CH4 reacts with = 2 mol of O2

1mol of CH4 produces = 1 mol of CO2

1mol of CH4 produces = 2 mol of H2O

Taking the assumption on the basis of stoichiometry is correct

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