The reaction of dinitrogen pentoxide with ammonia to form water vapor and nitrogen is hypothetical in the gas phase because at temperatures greater than 200k, dinitrogen pentoxide readil converts to crystalline ionic compound nitronium nitrate. Thus, it is feasible the the reaction could actually be run in NH3 (I) as a solvent at temperatures greater than 195k (melting point) and less than 240k (boiling point). Under these conditions how would the magnitude of Kc compare to 175 if all product H2O is dissvoled, why? Also, under these conditions how would a change in system pressure affect equilibrium for an identical change in pressure on the hypothetical system mentioned first?