(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T+0.5 x 10³T² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 105T-² Cp(HCI)/JK¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.

(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T+0.5 x 10³T² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 105T-² Cp(HCI)/JK¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.

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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