This industrial chemical reaction process generates nitrogen monoxide, an important component in the oxidation fo ammonia to nitric acid: 2 NO2 (g) → N2 (g) + 2 O2 (g) 2 CO (g) + O2 (g) → 2 CO2 (g) N2 (g) + O2 (g) → 2 NO (g) Calculate the ΔH°, ΔS°, ΔG°, and K (at 298 K) for each of the three steps in this industrial process.

Determine the sign of ΔSsys for the following chemical reactions without doing any calculations.  d) N2(g) + 3H2(g) → 2NH3(g)  ΔSsyse) KBr(s) → KBr(aq)  ΔSsysf) CO2(g) → CO2(aq)  ΔSsysg) Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)  ΔSsys

4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)     ΔrH = -1267 kJ mol-1 For the reaction above, select the correct sign for each of the following:   ΔSsurr  ΔSsys  ΔSuniv  Is the reaction spontaneous?

Which statement is INCORRECT with respect to thermodynamics? A) The sign of ΔG for a reaction is primarily determined by the sign of ΔH of the reaction.  B) The entropy of a perfect crystal at absolute zero is zero. C) Enthalpy can be thought of as the "heat content" of a system. D) For a reaction to be spontaneous, there must be an increase in the entropy of the universe. E) For a spontaneous reaction, the entropy of the reaction always increases.