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In the gaseous reactiojn 2A+B = A2B, Gibbs free energy=1200cal at 227Degree Celsius. What total pressure would be necessary to produce 60% conversion of B into A2B when 2:1 mixture is used? Ans (5.02atm) Sir, it is the question of "Modern Approach To chemical calculations" by Ramendra c. Mukerjee, page no.507, Q.no.31.
delG = -RT ln K. Find out K initially: say x moles of B is present, then 2x moels of A is present. Let total pressure be P. Finally: say a moles of B reacted. Then. 2a mol of A reacts and a mol of A2B is formed. given : a=0.6x. Hence, B- 0.4x and A - 1.2x and A2B= 0.6x partial pressure of A2B is (0.6/(0.6+1.2+0.4))*P = (0.6/2.2)P similarly Pb = (0.4/2.2)P, Pa = (1.2/2.2)P Kp = Pa2b / Pb .Pa 2 This value of Kp is obtained using the topmost formula. From this find out the value of P and that is the required value
delG = -RT ln K.
Find out K
initially:
say x moles of B is present, then 2x moels of A is present. Let total pressure be P.
Finally:
say a moles of B reacted. Then. 2a mol of A reacts and a mol of A2B is formed.
given : a=0.6x.
Hence, B- 0.4x and A - 1.2x and A2B= 0.6x
partial pressure of A2B is (0.6/(0.6+1.2+0.4))*P = (0.6/2.2)P
similarly Pb = (0.4/2.2)P, Pa = (1.2/2.2)P
Kp = Pa2b / Pb .Pa 2 This value of Kp is obtained using the topmost formula. From this find out the value of P and that is the required value
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