Chapter 3.6, Problem 3.42PP

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

a. to heat 5.25 g of water from 5.5 °C to 64.8 °C
b. lost when 75.0 g of water cools from 86.4 °C to 2.1 °C
c. to heat 10.0 g of silver from 112 °C to 275 °C
d. lost when 18.0 g Of gold cools from 224 °C to 118 °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

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