50. Using reference data (see appendix) on standard enthalpies of formation, standard entropies and standard Gibbs energies of formation, calculate for the reaction
NO2(g) H2(g)=N2(g) H2O(g)
at 298 K kJ/mol):
1) Heat of reaction (ΔrН298),
2) Change in entropy (ΔrS298),
3) Change in Gibbs energy (ΔrG298) (through enthalpy and entropy),
4) Value of the equilibrium constant (Kp).
Based on the obtained data, draw conclusions:
1) On the nature of the reaction (endothermic or exothermic),
2) On the direction of the reaction in an open system,
3) On the shift in chemical equilibrium with increasing temperature,
4) On the shift in chemical equilibrium with increasing pressure,
5) On the nature of the change in the equilibrium constant with increasing temperature.

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