For the experiment of Investigating Entropy Trail 1: NaOH: 2.037g, H2O: 50.038mL, inital temperature: 21.4°C, and final temperature: 29.2°C. Trail 2: NaOH: 2.074g, H2O: 50.017mL, inital temperature: 23.1°C, and final temperature: 30.9°C Trail 3: NaOH: 2.028g, H2O: 50.012mL, inital temperature: 22.9°C, and final temperature: 32.0°C Using the temperature measurements see you above, determine the average enthalpy change (kJ / m * ol) for the dissolution process. Here are the steps to do this for each dissolution: a. First find Delta*T for each b. Then find qsurroundings (remember q surroundings =q cal +q water) c. Then find q system (remember q system =-q sumoundings) d. Then find ∆H = Asystem moles salt dissolved
For the experiment of Investigating Entropy Trail 1: NaOH: 2.037g, H2O: 50.038mL, inital temperature: 21.4°C, and final temperature: 29.2°C. Trail 2: NaOH: 2.074g, H2O: 50.017mL, inital temperature: 23.1°C, and final temperature: 30.9°C Trail 3: NaOH: 2.028g, H2O: 50.012mL, inital temperature: 22.9°C, and final temperature: 32.0°C Using the temperature measurements see you above, determine the average enthalpy change (kJ / m * ol) for the dissolution process. Here are the steps to do this for each dissolution: a. First find Delta*T for each b. Then find qsurroundings (remember q surroundings =q cal +q water) c. Then find q system (remember q system =-q sumoundings) d. Then find ∆H = Asystem moles salt dissolved
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.98QP: When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and...
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For the experiment of Investigating Entropy
Trail 1: NaOH: 2.037g, H2O: 50.038mL, inital temperature: 21.4°C, and final temperature: 29.2°C.
Trail 2: NaOH: 2.074g, H2O: 50.017mL, inital temperature: 23.1°C, and final temperature: 30.9°C
Trail 3: NaOH: 2.028g, H2O: 50.012mL, inital temperature: 22.9°C, and final temperature: 32.0°C
Using the temperature measurements see you above, determine the average enthalpy change (kJ / m * ol) for the dissolution process. Here are the steps to do this for each dissolution:
a. First find Delta*T for each
b. Then find qsurroundings (remember q surroundings =q cal +q water)
c. Then find q system (remember q system =-q sumoundings)
d. Then find ∆H = Asystem moles salt dissolved
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