To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 10.6 g, and its initial temperature is -14.4 'C. The water resulting from the melted ice reaches the temperature of his skin, 31.0 "C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 10.6 g, and its initial temperature is -14.4 'C. The water resulting from the melted ice reaches the temperature of his skin, 31.0 "C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.

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...

See similar textbooks

Similar questions

7. How much heat is gained when the temperature of 288 g of liquid water is raised by 25 °C from room temperature at 25 °C ? a. 30 096 J b. 60 192 J c. 15 058 J d. 20 618 J e. oJ
Suggest a reason why the heat required to vaporize 102 g of water is so much higher than the heat required to heat 102 g of water through a temperature change of 75oC. Explain your answer.
Calculate the calorimeter constant for her calorimeter by following the steps below. 1. Calculate the mass of the warm water. 2. Calculate the change in temperature of the warm water. 3. Calculate the heat lost by the warm water. 4. Calculate the mass of the cold ocean water. 5. Calculate the change in temperature of the cold water. 6. Calculate the heat gained by the cold water. 7. Calculate the heat lost to the surroundings. 8. Calculate the calorimeter constant.
6. Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C. What was the initial temperature change of the ice? The specific heat capacity of H20(s) = 2.1 J/(g.°C).
25.7 g of ice at 0 C is converted to liquid water at the same temperature. How much heat is absorbed?
2. A 20.0 g sample of copper is heated from 20 °C to 1083 °C and half of it is melted at that temperature. The specific heat (sometimes referred to as the specific heat capacity) of copper is 0.385 J g¹K and the heat of fusion of copper is 205 Jg K. How much heat, in kJ, is absorbed by the sample of copper? A) 12.9 B) 8.91 C) 10.2 D) 5.18 E) 6.34
Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.
Examining ammonia (NH3) in a laboratory you find that compressing 90.4 g of that substance to a liquid releases 150.8 kJ of energy. Assuming all the energy transferred is due to compressing ammonia into a liquid, what is the heat of vaporization of ammonia?
You assumed that the initial temperature of the metal sample was the same as that of the boiling water. If the metal sample was actually at a lower temperature than the boiling water, how would your calculated value for the specific heat be affected?
The enthalpy for boiling water is 40.7 kJ/mol. What is the quantity of heat (in kJ) required to boil 418.1 g of water?