Q3. a) When 0.610 g of titanium (Ti) is combusted in a bomb calorimeter, the temperature of the calorimete increases from 25.00 °C to 50.50 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/°C. Calculate the heat of reaction for the combustion of Ti in kJ/mol Ti. (Mw(Ti): 47.87 g/mol) b) The value of AH° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) → 2HC1 (g) Calculate the value of AH°f for HCl (g) in kJ/mol.

Q3. a) When 0.610 g of titanium (Ti) is combusted in a bomb calorimeter, the temperature of the calorimete increases from 25.00 °C to 50.50 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/°C. Calculate the heat of reaction for the combustion of Ti in kJ/mol Ti. (Mw(Ti): 47.87 g/mol) b) The value of AH° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) → 2HC1 (g) Calculate the value of AH°f for HCl (g) in kJ/mol.

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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