Chapter 3: Matter and Energy
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1 Chapter 3: Matter and Energy
2 Convert between Fahrenheit, Celsius, and Kelvin temperature scales. Relate energy, temperature change, and heat capacity.
3 The atoms and molecules that compose matter are in constant random motion they contain thermal energy The temperature of a substance is a measure of its thermal energy.
4 The hotter an object, the greater the random motion of the atoms and molecules that compose it, and the higher its temperature.
5
6 Heat, which has units of energy, is the transfer or exchange of thermal energy caused by a temperature difference. when a piece of cold ice is dropped into a cup of warm water, heat (thermal energy) is transferred from the water to the ice.
7 Temperature, by contrast, is a measure of the thermal energy of matter (not the exchange of thermal energy). Measures the average kinetic energy of the molecules of matter.
8 Both cups of water are at the same temperature Which has a higher average kinetic energy? Which contains more thermal energy?
9 The Fahrenheit scale was set according to the following standards 0 F to the freezing point of a concentrated saltwater solution 96 F to normal body temperature.
10 On the Fahrenheit ( F) scale water freezes at 32 F water boils at 212 F Room temperature is approximately 72 F.
11 On the Celsius ( C) scale: water freezes at 0 C water boils at 100 C Room temperature is approximately 22 C
12 The Kelvin (K) scale avoids negative temperatures by assigning 0 K to the coldest temperature possible, absolute zero. Absolute zero is the temperature at which molecular motion stops. On the Kelvin (K) scale, water freezes at 273 K water boils at 373 K. Room temperature is approximately 295 K
13 The Fahrenheit degree is fiveninths the size of a Celsius degree. The Celsius degree and the Kelvin are the same size.
14 We can convert between Fahrenheit, Celsius, and Kelvin temperature scales using the following formulas:
15 Convert 25 C to kelvin.
16 Convert 358 K to Celsius.
17 Convert 55 F to Celsius.
18 Convert 139 C to Fahrenheit.
19 Convert 310 K to Fahrenheit.
20 Convert 321 F to kelvin.
21 Heat capacity: The quantity of heat (usually in joules) required to change the temperature of a given amount of the substance by 1 C
22 Specific heat capacity: the amount of heat required to raise the temperature of 1 g of any substance by 1 o C Specific heat capacity has units of joules per gram per degree Celsius, J/g C
23 Specific heat capacity is an intensive property! Specific heat describes how well an object retains heat A substance with a low specific heat is quickly heated, but also quickly cools A substance with a high specific heat takes a long time to warm up, but will also retain that heat for a longer period
24 Styrofoam is a very poor conductor of heat; it is a good insulator. It has a high specific heat. Metals are good conductors of heat. They have low specific heats.
25
26 If you want to heat a metal plate to as high a temperature as possible for a given energy input, what metal should you use? (Assume all the plates have the same mass.) a) copper b) iron c) aluminum d) it would make no difference
27 q is the amount of heat in joules. m is the mass of the substance in grams. C is the specific heat capacity in joules per gram per degree Celsius. T is the temperature change in Celsius. The symbol Δ means the change in, so ΔT means the change in temperature.
28 Gallium is a solid at 25.0 C and melts at 29.9 C. If you hold gallium in your hand, it can melt from your body heat. How much heat must 2.5 g of gallium absorb from your hand to raise its temperature from 25.0 C to 29.9 C? The specific heat capacity of gallium is J/g C.
29 The temperature of a lead fishing weight rises from 26 C to 38 C as it absorbs 11.3 J of heat. What is the mass of the fishing weight in grams?
30 A chemistry student finds a shiny rock that she suspects is gold. She determines that its mass is 14.3 g. She then finds that the temperature of the rock rises from 25 C to 52 C upon absorption of 174 J of heat. Find the heat capacity of the rock and determine whether the value is consistent with the heat capacity of gold (which is listed in Table 3.4).
31 A 328 g sample of water absorbs J of heat. Calculate the change in temperature for the water. If the water is initially at 25.0 C, what is its final temperature?
32 The heat capacity of substance A is twice that of substance B. If samples of equal mass of the two substances absorb the same amount of heat, which substance undergoes the larger change in temperature?
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