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1. The temperature of a 98.7 g piece of metal increases from 17.0 °C to 31.0 °C when the metal absorbs 705 J of heat. What is the specific heat of the metal?

1. The temperature of a 98.7 g piece of metal increases from 17.0 °C to 31.0 °C when the metal absorbs 705 J of heat. What is the specific heat of the metal?

Chemistry
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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HELP ME PLEASE!!!! REFER TO IMAGE ATTACHED SHOW ALL WORK PLEASE

MUST SHOW ALL WORK AND UNITS 1. The temperature of a 98.7 g piece of metal increases from 17.0 °C to 31.0 °C when the metal absorbs 705 J of heat. What is the specific heat of the metal? 2. The initial temperature of the water in a constant-pressure calorimeter is 25.0 °C. A reaction takes place in the calorimeter, and the temperature rises to 79.0 °C. The calorimeter contains 858 g of water, which has a specific heat of 4.18 J/g °C. Calculate the enthalpy change during this reaction. 3. C3H3 (g) + O2 (g) --> CO2 (g) + H20 (1) + 2220 KJ/mol Calculate the amount of heat required to burn 0.56 moles of C3H3. (must balance the equation first) 4. Calculate the amount of heat absorbed to liquefy 42.8 g of methanol (CH,0) at its melting point. The molar heat of fusion for methanol is 3.16 KJ/mol. 5. How much heat (in KJ) is absorbed when 75.7 g of methanol (CH,O) is converted to gas? Heat of vaporization for methanol is 35.2 KJ/mol.
Transcribed Image Text:MUST SHOW ALL WORK AND UNITS 1. The temperature of a 98.7 g piece of metal increases from 17.0 °C to 31.0 °C when the metal absorbs 705 J of heat. What is the specific heat of the metal? 2. The initial temperature of the water in a constant-pressure calorimeter is 25.0 °C. A reaction takes place in the calorimeter, and the temperature rises to 79.0 °C. The calorimeter contains 858 g of water, which has a specific heat of 4.18 J/g °C. Calculate the enthalpy change during this reaction. 3. C3H3 (g) + O2 (g) --> CO2 (g) + H20 (1) + 2220 KJ/mol Calculate the amount of heat required to burn 0.56 moles of C3H3. (must balance the equation first) 4. Calculate the amount of heat absorbed to liquefy 42.8 g of methanol (CH,0) at its melting point. The molar heat of fusion for methanol is 3.16 KJ/mol. 5. How much heat (in KJ) is absorbed when 75.7 g of methanol (CH,O) is converted to gas? Heat of vaporization for methanol is 35.2 KJ/mol.
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