4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal
4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal
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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4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C?
Answer: -550. cal (or -2.30 x 103 J)
5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C?
Answer: 3.00 x 103 cal (or 1.26 x 104 J)
6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C?
Answer: 92.4 cal
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