One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?

An aluminum rod 0.500 m in length and with a cross sectional area of 2.50 cm2 is inserted into a thermally insulated vessel containing liquid helium at 4.20 K. The rod is initially at 3(H) K. (a) If one-halt of the rod is inserted into the helium, how many liters of helium boil off by the time the inserted half cools to 4.20 K? Assume the upper half does not yet cool, (b) If the circular surface of the upper end of the rod is maintained at 300 K. what is the approximate boil-off rate of liquid helium in liters per second after the lower half has reached 4.20 K? (Aluminum has thermal conductivity of 3 100 YV/m K at 4.20 K; ignore its temperature variation. The density of liquid helium is 125 kg/m3.)

For a temperature increase of 10 at constant volume, what is the heat absorbed by (a) 3.0 mol of a dilute monatomic gas; (b) 0.50 mol of a dilute diatomic gas; and (c) 15 mol of a dilute polyatomic gas?

Can carbon dioxide be liquefied at room temperature (20 If so, how? If not, why not? (See the phase diagram in the preceding problem.)

In 1993, the U.S. government instituted a requirement that all room air conditioners sold in the United States must have an energy efficiency ratio (EER) of 10 or higher. The EER is defined as the ratio of the cooling capacity of the air conditioner, measured in British thermal units per hour, or Btu/h, to its electrical power requirement in watts. (a) Convert the EER of 10.0 to dimensionless form, using the conversion 1 Btu = 1 055 J. (b) What is the appropriate name for this dimensionless quantity? (c) In the 1970s, it was common to find room air conditioners with EERs of 5 or lower. State how the operating costs compare for 10 000-Btu/h air conditioners with EERs of 5.00 and 10.0. Assume each air conditioner operates for 1 500 h during the summer in a city where electricity costs 17.0 per kWh.

Consider an object with any one of the shapes displayed in Table 10.2. What is the percentage increase in the moment of inertia of the object when it is warmed from 0C to 100C if it is composed of (a) copper or (b) aluminum? Assume the average linear expansion coefficients shown in Table 16.1 do not vary between 0C and 100C. (c) Why are the answers for parts (a) and (b) the same for all the shapes?

Thus, -195.75 °C, 77.4 K, and -320.35 °F are equivalent temperatures on dif- ferent scales, (b) For a change ATc=[-100°C-(-195.75 °C)]=95.75 c°, we use Eq. 11.3 to find the change in temperature on the Fahrenheit scale as: ATF = ATC = ?I-100 - (-195.75)1 = 172.35 F Thus, a change 95.75 C° = 172.35 F, where the notations C° and F refer to temperature difference, not to be confused with actual temperatures, which are written in terms of symbols °C and °F. (1) The melting point of gold is 10640C and the boiling point is 26600C. (a) Express these temperatures in Kelvins. (b) Compute the difference of these temperatures in Celsius degrees and Kelvin degrees and compare the two numbers. (2) Liquid nitrogen has a boiling point of -195.810C at atmospheric pressure. Express this temperature in (a) degrees Fahrenheit, and (b) kelvins. ANS. (a) -3210F (b) 77.30C (3) A substance is heated from -120F to 1500F. What is its change in temperature on (a) the Celsius scale and (b) kelvin scale? ANS. (a)…

(a) You have a styrofoam container with 815 g of a soft drink (specific heat of 4,100 J/(kg · °C)) at 29.0° and you add a 60 g chunk of ice at 0°C. Assume the liquid and water mix uniformly as the ice melts and determine the final temperature of the mixture (in °C). 375.31 X Since the mixture is thermally isolated, the heat gained by the ice and the associated ice water is equal to the heat lost by the liquid. Write expressions for the heat gained by the ice as it changes from a solid to a liquid, gained by the ice water as it warms to the final temperature, and lost by the liquid as it cools to the final temperature. °C (b) What If? What is the minimum mass of the ice cube (in g) that will result in a final mixture at exactly 0°C? 290.1 g

(c) If melting ice of mass 80 g is added to 400 g of water at 20 °C, what will be the final temperature of the water, assuming that no energy is lost to the surroundings? The specific heat capacity of water is 4200 J kg °C'. The specific latent heat of fusion of ice is 3.34 × 10° J kg'.