(e) The mean bond enthalpy for chlorine is +242 kJ mol·' and that for fluorine is +158 kJ mol·'. The enthalpy of formation of CIF (g) is 56 kJ mol (i) Write down the formation reaction of CIF (g) and calculate a value for the bond enthalpy of the Cl-F bond. (ii) Calculate the enthalpy of formation of gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment, Explain.

(e) The mean bond enthalpy for chlorine is +242 kJ mol·' and that for fluorine is +158 kJ mol·'. The enthalpy of formation of CIF (g) is 56 kJ mol (i) Write down the formation reaction of CIF (g) and calculate a value for the bond enthalpy of the Cl-F bond. (ii) Calculate the enthalpy of formation of gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment, Explain.

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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