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 To determine the average enthalpy change (kJ / mol) for the dissolution process. a. Find Delta*T for each b. Find qsurroundings (remember q surroundings = qcal+qwater)
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 To determine the average enthalpy change (kJ / mol) for the dissolution process. a. Find Delta*T for each b. Find qsurroundings (remember q surroundings = qcal+qwater)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 78AP
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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
To determine the average enthalpy change (kJ / mol) for the dissolution process.
a. Find Delta*T for each
b. Find qsurroundings (remember q surroundings = qcal+qwater)
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