Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 5 - Thermochemistry - Exercises: 5.57

Answer

25.45 kJ/g

Work Step by Step

The heat capacity of the calorimeter is 7.854 kJ/C and the temperature changes from 23.44C to 30.57C. First we need to find the $\Delta T = 30.57C - 23.44C = 7.13 C$. Then we find the total amount of energy released by the quinone: 7.854 kJ/C * 7.13C = 55.999 kJ. Since we dissolved 2.200g of quinone then we have: 55.999kJ/2.2g = 25.45 kJ/g
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.