Unit IV 7. (a) How energy balance equation for adiabatic operation (b) 8. (a) (b) can be represented graphically? 10 Estimate the equilibrium constant at 600 K for the reaction At 298 K: C2H4(g) + H2O(g) → C₂H₂OH(g) At 298 K : AG° 2030 kcal/mol AF for H2O(g) = - 57798 cal/mol C2H5OH(g) = 56240 cal/mol = C2H4(g) 12496 cal/mol Discuss the General graphical procedure in detail. 10 The standard heat of gas phase reaction at 25°C =- (298 K) A+B →2R = 50000 J is Indicating that the reaction is strongly exothermic. It is planned to run this reaction at 1000 oC. What is the value of heat of reaction at this temperature? Is the reaction still exothermic at 1000°C. 5 5

Unit IV 7. (a) How energy balance equation for adiabatic operation (b) 8. (a) (b) can be represented graphically? 10 Estimate the equilibrium constant at 600 K for the reaction At 298 K: C2H4(g) + H2O(g) → C₂H₂OH(g) At 298 K : AG° 2030 kcal/mol AF for H2O(g) = - 57798 cal/mol C2H5OH(g) = 56240 cal/mol = C2H4(g) 12496 cal/mol Discuss the General graphical procedure in detail. 10 The standard heat of gas phase reaction at 25°C =- (298 K) A+B →2R = 50000 J is Indicating that the reaction is strongly exothermic. It is planned to run this reaction at 1000 oC. What is the value of heat of reaction at this temperature? Is the reaction still exothermic at 1000°C. 5 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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