What mass of water at 22.0°C must be allowed to come to thermal equilibrium with a 1:80 kg abe of aluminum initially at 150°C to lower the leimperature of the alurminum to 66.0°C? Assume any water turned to steam subsequently recondenses. kg Need Help? Read It

What mass of water at 22.0°C must be allowed to come to thermal equilibrium with a 1:80 kg abe of aluminum initially at 150°C to lower the leimperature of the alurminum to 66.0°C? Assume any water turned to steam subsequently recondenses. kg Need Help? Read It

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter4: The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 66P: A Carnot refrigerator exhausts heat to the air, which is at a temperature of 25 . How much is used...

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A 100-g piece of copper, initially at 95.0C, is dropped into 200 g of water contained in a 280-g aluminum can; the water and can are initially at 15.0C. What is the final temperature of the system? (Specific heats of copper and aluminum are 0.092 and 0.215 cal/g C. respectively.) (a) 16C (b) 18C (c) 24C (d) 26C (e) none of those answers
Calculate the length of a 1-meter rod of a material with thermal expansion coefficient a when the temperature is raised from 300 K to 600 K. Taking your answer as the new initial length, find the length after the rod is cooled back down to 300 K. Is your answer 1 meter? Should it be? How can you account for the result you got?
In car racing, one advantage of mixing liquid nitrous oxide (N2O) with air is that the boiling of the "nitrous" absorbs latent heat of vaporization and thus cools the air and ultimately the fuel-air mixture, allowing more fuel-air mixture to go into each cylinder. As a very rough look at this process, suppose 1.0 mol of nitrous oxide gas at its boiling point, 88 , is mixed with 4.0 mol of air (assumed diatomic) at 30 . What is the final temperature of the mixture? Use the measured heat capacity of N2O at 25 , which is 30.4J/mol . (The primary advantage of nitrous oxide is that it consists of 1/3 oxygen, which is more than air contains, so it supplies more oxygen >to bum the fuel. Another advantage is that its decomposition into nitrogen and oxygen releases energy in the cylinder.)
Unreasonable results. (a) Find the temperature of 0.360 kg of water, modeled as an ideal gas, at a pressure of 1.01105 Pa if it has a volume of 0.615 m3. (b) What is unreasonable about this answer? How could you get a better answer?
A car tile contains 0.0380 m3 of air at a pressure of 2.20105 Pa (about 32 psi). How much more internal energy does this gas have than the same volume has at zero gauge pressure (which is equivalent to normal atmospheric pressure)?
A Carnot refrigerator exhausts heat to the air, which is at a temperature of 25 . How much is used by the refrigerator if it freezes 1.5 g of water per second? Assume the water is at 0 .
When our bodies get too warm, they respond by sweating and increasing blood circulation to the surface to transfer thermal energy away from the core. What effect will those processes have on a person in a 40.0 hot tub?
Most automobiles have a coolant reservoir to catch radiator fluid than may overflow when 1he engine is hot. A radiator is made of copper and is filled to its 16.0L capacity when at 10.0C. What volume of radiator fluid will overflow when the radiator and fluid reach their 95.0C operating temperature, given that the fluid’s volume coefficient of expansion is =400106/C ? Note that this coefficient is approximate, because most car radiators have operating temperatures of greater than 95.0C.
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?
One might think that the internal energy of diatomic gases is given by Eint=5RT/2 . Do diatomic gases near room temperature have more or less internal energy than that? Hint: Their internal energy includes the total energy added in raising the temperature from the boiling point (very low) to room temperature.
A tank contains 111.0 g chlorine gas l2), which is at temperature 82.0 and absolute pressure 5.70105 Pa. The temperature of the air outside the tank is 20.0 . The molar mass of Cl2 is 70.9 g/mol. (a) What is the volume of the tank? (b) What is the internal energy of the gas? (c) What is the work done by the gas if the temperature and pressure inside the tank drop to 31.0 and 3.80105 Pa, respectively, due to a leak?
In some countries, liquid nitrogen is used on daily trucks instead of mechanical refrigerators. A 3.00-hour delivery trip requires 200 L of liquid nitrogen, which has a density of 808 kg/m3. (a) Calculate the heat transfer necessary to evaporate this amount of liquid nitrogen and raise its temperature to 3.00 . (Use cp and assume it is constant over the temperature range.) This value is the amount of cooling the liquid nitrogen supplies. (b) What is this heat transfer rate in kilowatt-hours? (c) Compare the amount of cooling obtained from melting an identical mass of 0- ice with that from evaporating the liquid nitrogen.