Chapter 3.6, Problem 3.40PP

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

a. calories lost when 85 g of water cools from 45 °C to 25 °C
b. joules to heat 75 g of water from 22 °C to 66 °C
c. kilocalories to heat 5.0 kg of water from 22 °C to 28 °C
d. kilojoules to heat 224 g of gold from 18 °C to 185 °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

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