a) At high temperature, ammonia reduces copper(II) oxide to the free metal: Step

Question

1. a) At high temperature, ammonia reduces copper(II) oxide to the free metal:
   Step 1: 2NH3(g) + 6CuO(s) => N2(g) + 3Cu2O(s) + 3H2O(g)
   Step 2: 2NH3(g) + 3Cu2O(s) => N2(g) + 6Cu(s) + 3H2O(g) Appendix C to calculate the heat of reaction for Step 1. a.

a) At high temperature, ammonia reduces copper(II) oxide to the free metal:
Step 1: 2NH3(g) + 6CuO(s) => N2(g) + 3Cu2O(s) + 3H2O(g)
Step 2: 2NH3(g) + 3Cu2O(s) => N2(g) + 6Cu(s) + 3H2O(g) Appendix C to calculate the heat of reaction for Step 1. a. a) At high temperature, ammonia reduces copper(II) oxide to the free metal:
Step 1: 2NH3(g) + 6CuO(s) => N2(g) + 3Cu2O(s) + 3H2O(g)
Step 2: 2NH3(g) + 3Cu2O(s) => N2(g) + 6Cu(s) + 3H2O(g) Appendix C to calculate the heat of reaction for Step 1. a.

Explanation / Answer

?Hproducts -?Hreactants

2NH3(g) 2(-80.8)

6CuO(s) 6(?156)

= -1097.6

N2(g) 0 in standard state

3Cu2O(s) 3(?170 )

3H2O(g) 3(-241.818)

=-1235.454

-1235.454 - -1097.6 = -137.845 kj/mol

2.The ?H of formation of CO2 is -393.5-kJ/mol. If 6043-kJ of thermal energy is produced, then 6043kJ / 393-kj/mol = 15.37 moles of carbon = ( 15.37 mol x 12-g/mol = 184.51 g of carbon) was consumed

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