The equilibrium constant. Kc, is calculated using molar concentrations. For gase

Question

The equilibrium constant. Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant. Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = Kc (KT) Delta n where R = 0.08206 L middot atm /(K middot mol) , T is the absolute temperature, and Delta n is the change in the number of moles of gas. For example, consider the reaction N2(g) + 3H2(g) 2NH3(g) for which Delta n = 2 - (1 + 3) = -2. For the reaction 2A(g) + 2B(g) C(g) Kc = 64.5 at a temperature of 115 degree C. Calculate the value of Kp. Express your answer numerically. For the reaction X(g) + 3Y(g) 3Z(g) Kp = 33.4 at a temperature of 31 degree C. Calculate the value of Kc. Express your answer numerically.

Explanation / Answer

We Know that :     The given Reaction is :       2 A ( g ) + 2B ( g ) <------- > C ( g )          Kp = Kc ( RT ) ng            ng = 1 - 4                     = -3          Kp =   64.5 ( 0.0821 x 388 )-3                   = 0.001995 b.             X ( g )   + 3 Y ( g ) <---------> 3 Z ( g )                   Kp = Kc ( RT ) ng            ng =  3 - 4                     = -1           33.4 =   Kc ( 0.0821 x 304 )-1                   = 833.6105                                      = 0.001995 b.             X ( g )   + 3 Y ( g ) <---------> 3 Z ( g )                   Kp = Kc ( RT ) ng            ng =  3 - 4                     = -1           33.4 =   Kc ( 0.0821 x 304 )-1                   = 833.6105                               ng =  3 - 4                     = -1           33.4 =   Kc ( 0.0821 x 304 )-1                   = 833.6105                                      = 833.6105                   

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