For reactions çarried out under standard-state conditions, the equation AG= AH- TAS becomesAG =H - TAS".TAS .Assuming AH and AS%3Dare independent of temperature, one can derive theequation:K2In-K1AHT2- T1.%3DRwhere K and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, K, is4.63 x 10 for the reactionN204g) 5 2NO28)AH= 58.0 kJ/molcalculate the equilibrium constant at 63.0°C.Kc%3D

The given relation is, lnK2K1=∆HoRT2-T1T1T2 Where, K1 and K2 are the equilibrium…

For reactions carried out under standard-state conditions, the equation AG= AH- TAS becomes AG =H - TAS.Assuming AH and AS equation: are independent of temperature, one can derive the K2 AH T2-T1 In- K1 R where K and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, K, is 4.63 x 103 for the reaction N204(g) 5 2NO2(g) AH = 58.0 kJ/mol calculate the equilibrium constant at 63.0°C. K =

For reactions carried out under standard-state conditions, the equation AG= AH- TAS becomes AG =H - TAS.Assuming AH and AS equation: are independent of temperature, one can derive the K2 AH T2-T1 In- K1 R where K and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, K, is 4.63 x 103 for the reaction N204(g) 5 2NO2(g) AH = 58.0 kJ/mol calculate the equilibrium constant at 63.0°C. K =

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...

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