The species H and O can react to form either pure HO, pure HO or a...

 

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The species H and O can react to form either pure HO, pure HO or a mixture of the two, depending on the conditions (temperature, pressure, catalyst, etc). These reactions are shown conceptually below. 1.aH2(g)+bO2(g) CH0(1) 2. dH (g) +eO2 (9) fHO (1) 3. gH(g) + hO2(g) iHO(l) +jHO (1) For the 3 reactions above please answer the questions below a) Find the stoichiometric coefficients of the reactants for each reaction independently, assuming that 1 mole of (each) product is formed. b) Assume there is a specific catalyst that catalyzes the reaction #3, in such a way that the ratio of ij is 9:1. Assuming the reaction goes to completion, what are the values of g and h? c) Invert the product ratio in part b to be 1:9. What are the values of g and h now? d.) Which of the three reactions (1,2, or 3) can result in the complete consumption of all reactants if there is an equimolar feed (i.e. H:0 = 1:1) to a reactor? For the one(s) that cannot consume all reactants, calculate the ratio between the unspent reactant and product(s), assuming the limiting reactant is totally consumed. The species H and O can react to form either pure HO, pure HO or a mixture of the two, depending on the conditions (temperature, pressure, catalyst, etc). These reactions are shown conceptually below. 1.aH2(g)+bO2(g) CH0(1) 2. dH (g) +eO2 (9) fHO (1) 3. gH(g) + hO2(g) iHO(l) +jHO (1) For the 3 reactions above please answer the questions below a) Find the stoichiometric coefficients of the reactants for each reaction independently, assuming that 1 mole of (each) product is formed. b) Assume there is a specific catalyst that catalyzes the reaction #3, in such a way that the ratio of ij is 9:1. Assuming the reaction goes to completion, what are the values of g and h? c) Invert the product ratio in part b to be 1:9. What are the values of g and h now? d.) Which of the three reactions (1,2, or 3) can result in the complete consumption of all reactants if there is an equimolar feed (i.e. H:0 = 1:1) to a reactor? For the one(s) that cannot consume all reactants, calculate the ratio between the unspent reactant and product(s), assuming the limiting reactant is totally consumed.

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a For reaction 1 1 mole of H2O is formed so a 1 b 0 For reaction 2 1 mole of H2O2 is formed so d 1 e ... View the full answer