Consider the following reaction which occurs at constant temperature and pressur

Question

Consider the following reaction which occurs at constant temperature and pressure:
2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) H = -664.4 kJ

Which has the higher enthalpy, 2 NO(g) + 2 H2(g) or N2(g) + 2 H2O(g)?

2 NO(g) + 2 H2(g)
N2(g) + 2 H2O(g)




Without referring to tables indicate which of each of the pairs of choices below has the higher enthalpy:



(a)
carbon dioxide and water resulting from the complete combustion of one mole of gasoline
1 mole of gasoline mixed with a stoichiometrically equivalent amount of oxygen




(b)
1 mol of H2O(l) at 0 oC
1 mol of H2O(s) at 0 oC




(c)
1 mol of N2(g) at -100 oC
1 mol of N2(l) at -100 oC




(d)
1 mol of H2(g) and 0.5 mol of O2(g) at 25 oC
1 mol of H2O(g) at 25 oC

Explanation / Answer

(c) 1 mol of N2(g) at -100 oC 1 mol of N2(l) at -100 oC

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