We will list the various quantities in the columns headed by the compound formulas. Let n...

Transcribed Image Text:

We will list the various quantities in the columns headed by the compound formulas. Let n° be the number of moles of N2O4, and Ee the progress of the reaction at equilibrium, à̟the dissociated fraction at equilibrium à = /n° %3D N,O4 + 2 NO,2(3) Stoichiometric coefficient -1 +2 Number of initial moles , n n° Number of moles at equilibrium n° - E. 0 + 2, De Total number of moles n= n° + , mole fraction , X, n° - , / 2 , / n° + E, n° - . c As = {/n°, the X, are 1 - à, / 2, à/ 1+ à, 1 + à. Partial pressures p.xp (1- à,/) ( 2 à/) (1 + à) (1+ à) using the values of the partial pressures we obtain = p? NO,/pN, 0, = 4à,'p/(1-à²,) Developing à = (K,/K, + 4p)/2 Question: Do the same work for the equilibrium: + 2(g) 3 H218) 2 NH313) 2(g) 3(g) Assume the initial moles equal to the stoichiometric coefficients We will list the various quantities in the columns headed by the compound formulas. Let n° be the number of moles of N2O4, and Ee the progress of the reaction at equilibrium, à̟the dissociated fraction at equilibrium à = /n° %3D N,O4 + 2 NO,2(3) Stoichiometric coefficient -1 +2 Number of initial moles , n n° Number of moles at equilibrium n° - E. 0 + 2, De Total number of moles n= n° + , mole fraction , X, n° - , / 2 , / n° + E, n° - . c As = {/n°, the X, are 1 - à, / 2, à/ 1+ à, 1 + à. Partial pressures p.xp (1- à,/) ( 2 à/) (1 + à) (1+ à) using the values of the partial pressures we obtain = p? NO,/pN, 0, = 4à,'p/(1-à²,) Developing à = (K,/K, + 4p)/2 Question: Do the same work for the equilibrium: + 2(g) 3 H218) 2 NH313) 2(g) 3(g) Assume the initial moles equal to the stoichiometric coefficients