A coffee-cup calorimeter contains 70 mL of water with an initial temperature of 24.9°C. An unknown sample with a mass of 6.259 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 86.4°C. (Water: density = 1g/mL; specific heat = 4.184 J/g-°C). 1. How much heat (in Joules) was absorbed by the water in the calorimeter?_________ (Write your answer in 2 decimal places without the unit).
A coffee-cup calorimeter contains 70 mL of water with an initial temperature of 24.9°C. An unknown sample with a mass of 6.259 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 86.4°C. (Water: density = 1g/mL; specific heat = 4.184 J/g-°C). 1. How much heat (in Joules) was absorbed by the water in the calorimeter?_________ (Write your answer in 2 decimal places without the unit).
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A coffee-cup calorimeter contains 70 mL of water with an initial temperature of 24.9°C. An unknown sample with a mass of 6.259 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 86.4°C.
(Water: density = 1g/mL; specific heat = 4.184 J/g-°C).
1. How much heat (in Joules) was absorbed by the water in the calorimeter?_________ (Write your answer in 2 decimal places without the unit).
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