As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of NH3 reacted. Explain. As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant volume and temperature, the total pressure increases by some factor. Why the increase in pressure and by what factor does the total pressure increase when reactants are completely converted into products? How do the partial pressures of the product gases compare to each other and to the initial pressure of NH3?
2/16/16 Volatile Solute and Raoult s La P A = XAP(degrees) B P B= X A P(degrees) B P T= P A + PB B.P. elevation: (delta)Th = i(Kb)m (delta)b= Tb — T(degrees) b * (delta)Th — change in b.p. * K b— b.p. elevation constant * m — molality * Tb — new b.p. * b— pure b.p. T(degrees) F.P. depression: (delta)T f = i(f)m (deltaf= T(degrees) f— T f i van’t Hoff factor —> number of particles Nonelectrolytes: CH3CH2OH (l) —> CH3CH2OH (aq) i = 1 C6H12O6 (s) —> C6H12O6 (aq) i = 1 i = 2 NaCl (s) —> Na+ (aq) + Cl— (aq) i = 4 Na3PO4 (s) —> 3Na+ (aq) + PO4 ^ 3 (aq) i = 3 BaCl2 (s) —> Ba ^ 2+ (aq) + 2Cl— (aq) Electrolytes (strong acids): HCl hydrochl