Ammonia gas at a pressure of $$20$$ atm and $$27$$°C is heated in a constant volume in a container to a temperature of $$327$$°C at which new pressure becomes $$50$$ atm and the following equilibrium $$2NH3g$$⇌ $$N2g+3H2gis$$ established. Percentage dissociation of ammonia at this temperature is $$X2$$. The value of is

Question

Ammonia gas at a pressure of $$20$$ atm and $$27$$°C is heated in a constant volume in a container to a temperature of $$327$$°C at which new pressure becomes $$50$$ atm and the following equilibrium $$2NH3g$$⇌ $$N2g+3H2gis$$ established. Percentage dissociation of ammonia at this temperature is $$X2$$. The value of  is

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Given, Pressure, $$p1=20atmPressure$$, $$p2=50atmTemperature$$,$$T1=270C+$$ $$2730C=300$$ kTemperature,$$T2=3270C+$$ $$2730C$$ $$=$$ $$600$$ k Reaction,  $$2NH3(g)$$  ⇌   $$N2(g)$$  $$+$$ $$3H2(g)After$$ dissociation  $$1-$$α                                      α$$2$$                          $$3$$α$$2$$ Totalmoles $$=$$ $$1+$$αIdeal gas equation,⇒$$PV=nRT$$⇒$$20$$ $$V50$$ V  $$=$$  $$1$$  R  $$300n$$  R  $$600$$⇒n $$=$$ $$1.25$$⇒α $$=$$ $$0.25$$⇒% $$=$$ $$25$$ i.e. $$x=5$$

Ammonia gas at a pressure of 20 atm and 27°C is heated in a constant volume in a container to a temperature of 327°C at which new pressure becomes 50 atm and the following equilibrium 2NH3g⇌ N2g+3H2gis established. Percentage dissociation of ammonia at this temperature is X2. The value of is

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