The Bosch reaction reduces CO_2 using hydrogen gas to produce elemental carbon a

Question

The Bosch reaction reduces CO_2 using hydrogen gas to produce elemental carbon and water vapor. The table on the right provides heats of formation of some of the substances that are relevant to the problem below. Write a balanced equation for this reaction with phases noted. Use the provided heats of formation to calculate Delta H degree (kJ) for this reaction. Under what temperature conditions, if any, would this reaction be spontaneous? One way in which spacecraft could regenerate oxygen from the water produced by the Bosch reaction is to convert the water vapor by the water splitting reaction 2H_2O(g) 2H_2(g) + O_2(g) Give 3 ways to maximize the conversion to products with explanation using lessthanorequalto Chatelier's principle

Explanation / Answer

Bosch process

(a) balanced equation,

CO2(g) + 2H2(g) --> C(s) + H2O(g)

(b) dHorxn = dHo(products) - dHo(reactants)

                 = (2 x -241.82) - (-393.51) = -90.13 kJ/mol

(c) The reaction would be spontaneous at high temperature conditions above 500 oC.

(d) 2H2O(g) <==> 2H2(g) + O2(g)

According to LeChatellier's principle,

To increase the products

a) increase the H2O concentration : More reactants would force equilibrium towards right handside to reestablish equilibrium condition.

b) decrease H2 or O2 concentration : As products get less, equilibrium is disturbed, more reactant would form products to reequilibriate.

c) decrease pressure : The reaction would shift in the direction which has more gaseous molecules.

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