Question: Consider the Haber process: N2(g) + 3H2(g) 2NH3(g); H = 91.8 kJ The density of ammonia at 25oC and 1.00 atm is 0.696 g/L.

Consider the Haber process:
N2(g) + 3H2(g) → 2NH3(g); ∆H° = –91.8 kJ
The density of ammonia at 25oC and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol•oC). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25oC and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25oC to 400oC, the temperature at which the Haber process is run?

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