Exam 12: Thermal Properties of Matter

A 5.3 L flask of ideal neon gas (which is monatomic)is at a pressure of 6.0 atm and a temperature of $290 \mathrm {~K} .$ The atomic mass of neon is 20.2 g/mol. What is the mass of the neon gas in the flask. (R = 8.31 J/mol ? K, 1 atm = 101 kPa, N_A = 6.022 × 10²³ molecules/mol)

A 600-g piece of iron at 100°C is dropped into a calorimeter of negligible heat capacity containing 100 g of ice at 0°C and 120 g of water, also at 0°C. What is the final temperature of the system? The specific heat of iron is 448 J/kg ∙ K, the latent heat of fusion of water is 33.5 × 10⁴ J/kg, and the specific heat of water is 4186 J/kg ∙ K.

If the temperature of an ideal gas is increased from 20°C to 40°C, by what percent does the speed of the molecules increase?

It is necessary to determine the specific heat of an unknown object. The mass of the object is $201.0 \mathrm {~g}$ It is determined experimentally that it takes $15.0 \mathrm {~J}$ to raise the temperature $10.0 ^ { \circ } \mathrm { C }$ What is the specific heat of the object?

If you add 700 kJ of heat to 700 g of water originally at 70.0°C, how much water is left in the container? The latent heat of vaporization of water is 22.6 × $10 ^ { 5 }$ J/kg, and its specific heat capacity is 4186 J/kg ? K.

A quantity of mercury occupies 400.0 cm³ at 0°C. What volume will it occupy when heated to 50°C? Mercury has a volume expansion coefficient of 180 × 10^-6 K^-1.

The coefficient of linear expansion of steel is 12 × 10^-6 K^-1. What is the change in length of a 25-m steel bridge span when it undergoes a temperature change of 40 K from winter to summer?

An oxygen molecule, O₂, falls in a vacuum. From what height must it fall so that its translational kinetic energy at the bottom of its fall equals the average translational kinetic energy of an oxygen molecule at 920 K? The mass of one O₂ molecule is 5.312 × 10^-26 kg, and the Boltzmann constant is 1.38 × 10^-23 J/K. Neglect air resistance and assume that g remains constant at 9.8 m/s² throughout the fall of the molecule.

The figure shows a pV diagram for an ideal gas that is carried around a cyclic process. How much work is done in one cycle if p₀ = $4.00 \mathrm {~atm}$ and $V _ { 0 } = 3.00$ L? (1.00 atm = 101 kPa)

The rms speed of a certain sample of carbon dioxide molecules, with a molecular weight of 44.0 g/mole, is 396 m/s. What is the rms speed of water vapor molecules, with a molecular weight of 18.0 g/mol, at the same temperature as the carbon dioxide?

Heat is added to a 3.0 kg piece of ice at a rate of $636.0 \mathrm {~kW}$ How long will it take for the ice at 0.0° C to melt? For water L_F = 334,000 J/kg and L_V = 2.246 × 10⁶ J/kg.

The temperature of an ideal gas in a sealed rigid 0.60- $m ^ { 3 }$ container is reduced from 460 K to $270 \mathrm {~K}$ The final pressure of the gas is $90 \mathrm { kPA } .$ The molar heat capacity at constant volume of the gas is 28.0 J/mol ? K. How much heat is absorbed by the gas during this process? (R = 8.31 J/mol ? K)

Two metal rods are to be used to conduct heat from a region at 100°C to a region at 0°C as shown in the figure. The rods can be placed in parallel, as shown on the left, or in series, as on the right. When steady state flow is established, the heat conducted in the series arrangement is

A container with rigid walls is filled with 4.00 mol of air at 17°C with C_V = 2.5R. What is the final temperature of the air if its internal energy is increased by 28 kJ? (R = 8.31 J/mol ∙ K)

Object 1 has three times the specific heat capacity and four times the mass of Object 2. The two objects are heated from the same initial temperature, T₀, to the same final temperature T_f. During this process, if Object 1 absorbs heat Q, the amount of heat absorbed by Object 2 will be

Your lungs hold 4.2 L of air at a temperature of 27°C and a pressure of 101.3 kPa. How many moles of air do your lungs hold? (R = 8.31 J/mol ∙ K)

The process in which heat flows by the mass movement of molecules from one place to another is known as

A piece of iron of mass 0.12 kg is taken from an oven where its temperature is 336°C and quickly placed in an insulated copper can that contains 0.20 kg of water. The copper can has mass 0.50 kg, and it and the water in it are originally at a temperature of 20°C. Calculate the final temperature of the system, assuming no heat is lost to the surroundings. Use the following specific heats: 4190J/kg ? C° (water), 470 J/kg ? C° (iron), and 390 J/kg ? C° (copper).

How many grams of ice at -17°C must be added to 741 grams of water that is initially at a temperature of $70 ^ { \circ } \mathrm { C }$ to produce water at a final temperature of $12 ^ { \circ } \mathrm { C } ?$ Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg ? C° and of ice is 2000 J/kg ? C°. For water the normal melting point is 0°C and the heat of fusion is 334 × 10³ J/kg. The normal boiling point is 100°C and the heat of vaporization is 2.256 × 10⁶ J/kg.

When a gas expands adiabatically,