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?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.27QP: Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB....
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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?
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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