Chapter 3.6, Problem 3.37QAP

Use the heat equation to calculate the energy, in joules and calories, for each of the following (see TABLE3.11):

a. to heat 25.0 g of water from 12.5 °C to 25.7 °C
b. to heat 38.0 g of copper from 122 °C to 246 °C
c. lost when 15.0 g of ethanol, C₂H₆O, cools from 60.5 °C to −42.0 °C
d. lost when 125 g of iron cools from 118 °C to 55 °C

TABLE 3.11 Specific Heats for Some Substance

Substance	$\text{cal}/\text{g}\text{°C}$	$\text{J}/\text{g}\text{°C}$
Elements
Aluminum, Al(s)	0.214	0.897
Copper, Cu(s)	0.0920	0.385
Gold, Au(s)	0.0308	0.129
Iron, Fe(s)	0.108	0.452
Silver, Ag(s)	0.0562	0.235
Titanium, Ti(s)	0.125	0.523
Compounds
Ammonia, NH3(g)	0.488	2.04
Ethanol, C2H6O(?)	0.588	2.46
Sodium chloride, NaCl(s)	0.207	0.864
Water, H2O(?)	1.00	4.184
Water, H2O(s)	0.485	2.03

$\text{specific heat }(SH)=\frac{\text{heat}}{\text{mass }\Delta T}=\frac{\text{cal}(\text{or J)}}{\text{g °C}}$