Chapter 3.6, Problem 3.39PP

Use the heat equation to calculate the energy for each of the following (see TABLE3.11):

a. calories to heat 8.5 g Of water from 15 °C to 36 °C
b. joules lost when 25 g Of water cools from 86 °C to 61 °C
c. kilocalories to heat 150 g of water from 15 °C to 77 °C
d. kilojoules to heat 175 g of copper from 28 °C to 188 °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

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