0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 4.21 °C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･ °C and the density of the solution is 1.02 g/mL).
0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 4.21 °C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･ °C and the density of the solution is 1.02 g/mL).
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 127CWP: In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0...
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0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 4.21 °C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･ °C and the density of the solution is 1.02 g/mL).
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