Thermochemistry

Heat Capacity

Part 1

Read Section 4.4 (including 4.4a and 4.4b) in your textbook.  To use the direct link to the section in your etext provided below, first log into your CengageBrain account and then click the link.

http://east.instructor.cengagenow.com/ilrn/covalent/ebookRedirect.do?eISBN=9781285460321&contentId=MYIOSC118770849


A key idea from Section 4.4 is the relationship:

q = C x m x ΔT, where

q is the heat in J
C is the specific heat capacity in J/[g⋅°C]
m is the mass in g
ΔT is the temperature change in either °C or K

Notice that when a substance’s temperature increases (ΔT > 0), the resulting value for q will be positive (corresponding to energy flow into the substance).  Conversely, a drop in a substance’s temperature (ΔT < 0) results in a negative value for q (energy flow out of substance).

Part 2

Suppose you have 3 cubes of metal – aluminum, copper, and iron – each with a mass of 20.0 g.   Heat is applied such that each cube absorbs the same amount of heat as the others.  Use the specific heat capacity values given in Table 4.1 to answer the following questions.

[table “1” not found /]

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