Calculate the Entalphy of Combustion: Calorimeter constant C from part A q = -0.23 J Tf - TI = ΔT 26.47°C-20°C ΔT= 6.47°C q/°c = -0.23 J/6.47°C = 0.04J/°C The calorimeter constant C = 0.04 J/°C Mass of the Metals MgO- 40.3044 grams k- 39.10 grams HCL- 36.5 grams/100 ml of 1 mole of HCL Questions: (B.3) Using the equation in B3 and your calorimeter constant C from Part A, calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole. • K+HCL → KCL+H2
Calculate the Entalphy of Combustion: Calorimeter constant C from part A q = -0.23 J Tf - TI = ΔT 26.47°C-20°C ΔT= 6.47°C q/°c = -0.23 J/6.47°C = 0.04J/°C The calorimeter constant C = 0.04 J/°C Mass of the Metals MgO- 40.3044 grams k- 39.10 grams HCL- 36.5 grams/100 ml of 1 mole of HCL Questions: (B.3) Using the equation in B3 and your calorimeter constant C from Part A, calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole. • K+HCL → KCL+H2
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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Calculate the Entalphy of Combustion:
Calorimeter constant C from part A
q = -0.23 J
Tf - TI = ΔT
26.47°C-20°C
ΔT= 6.47°C
q/°c = -0.23 J/6.47°C = 0.04J/°C
The calorimeter constant C = 0.04 J/°C
Mass of the Metals
MgO- 40.3044 grams
k- 39.10 grams
HCL- 36.5 grams/100 ml of 1 mole of HCL
Questions:
(B.3) Using the equation in B3 and your calorimeter constant C from Part A, calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole.
• K+HCL → KCL+H2
ΔHb = _______________________
(B.4) Similarly, calculate ΔH for the reaction involving MgO and HCL.
• MgO(s)+ 2HCl(aq) →MgCl2(aq)+ H2O(l)
ΔH = _______________________
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