Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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This and the following questions pertain to the following problem: In this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. Now that we have the enthalpy of reaction, q (reaction) = – 1390.399457 J, and the number of moles 0.035491131 mol SrCl2 , we can get the enthalpy of reaction. Give Delta H (rxn) in correct sig figs.
Delta H (rxn) = q / n = – 1390.399457 J / 0.035491131 mol SrCl2
Delta H (rxn) = – 39175.96895 J / mol SrCl2
Delta H (rxn) = – 39.17596895 kJ / mol SrCl2
Select one:
a. none of these
b. – 39.17596895 kJ / mol
c. – 39 kJ / mol
d. – 4 x 10^1 kJ / mol
e. – 39.18 kJ / mol
f. – 39.1 kJ / mol
g. – 39.17 kJ / mol
h. – 39.2 kJ / mol
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