Question

At 25°C the equilibrium constant (Kp) for following reaction is 4.5% 10% the 2NO(g) = No (9) + Oo (9) _ If the initial pressure of NO cg) befor any products have I been formed is 9.5 atm, what are the equilibrium partial pressures of Na(g), O2 (g), and Norg) ?

Answer 1

A4 280, constant (Kp = Equilibrium 4.5x10t 2NO(g) = N269) + Oz (9) Inhal tzo 9.5 At 9.5-2 p Equilibrium e r Kp = (P.2) (Por) . (PND)? 4.5X107 = Kp = p XP (9.5-2P) 2 atmyatim (atm) 4. 5x107 =p2 (9.5-26) 2 s = 5.5x107 = 45 X 106 9.5-2P P 9.5-20 = 6.708103 P = 9.5x 6.70X -2 X6.7 X1 X P = 63650 1340op 13401P =63650 P= 4.749 1 P=4.75 atm anned with im Scanner

Per suro of N (P) = q.75 atm Preasure of o2 (P) = 4.75 atm Preasure of Nola = z 9.5-2P 9.5 – 2X4075 9.5-go5 zo atm

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acc to the data give in question .I have solved the question ...bt how the partial pressure of NO(g) at equilibrium is zero..if it is zero then no equilibrium is there..so check ur data once ...i have provided solution how to solve the ques ..based on that correct the question if given data is wrong..i hope this will help u ..thank u so much