An insulated container holds m = 5.23 kg of the solid form of a substance right at the melting temperature of 229.7 K (think "ice"). It isconnected to an insulated container that contains the vapour form of the same substance (think "steam") in such a way that heat can transferbetween the two containers, but not with the environment. The vapour is exactly at the vapourization temperature of 301.6 K, and thecontainer has exactly enough vapour so that the moment the solid portion has finished melting, exactly all of the vapour has finishedcondensing. The latent heat of fusion of the substance is 46850 J/kg and the latent heat of vapourization of the substance is 73380 J/kg.What is the total change in entropy for the substance in both containers combined? (i.e. what is AS solid + AS vapour)J/K

Answered: Image /qna-images/answer/3e995a93-a496-46bc-bf47-6c6810c158de.jpg

Answered: An insulated container holds m = 5.23…

Similar questions

What is the average kinetic energy (in J) of hydrogen atoms on the 5500°C surface of the sun? What is the average kinetic energy (in J) of helium atoms in a region of the solar corona where the temperature is 6.70 ✕ 105 K?
In an experiment, a 0.160-kg piece of ceramic superconducting material at 17 °C is placed in liquid nitrogen at its boiling point (−195.8 °C) to cool. The nitrogen is in a perfectly insulated flask that allows the gaseous N2 to escape immediately. How much mass of liquid nitrogen will be boiled away? (Take the specific heat of the ceramic material to be the same as that of glass.)
The total internal kinetic energy of 5 gallons of water is 2x10^8 J. The total kinetic internal energy of the water in a 100,000 gallon swimming pool is 5x10^11J. How many water molecules are in the 5 gallon water? Which body of water is at higher temperature?
A 283 g silver figure of a polar bear is dropped into the 249 g aluminum cup of a well-insulated calorimeter containing 265 g of liquid water at 20.9°C. The bear's initial temperature is 98.5°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/ (kg-K), 910 J/ (kg-K), and 4190 J/ (kg-K). final temperature: °C
Scientists experiment with a balloon near a Himalayan fresh water lake at an altitude of 5000 m where atmospheric pressure is half of that at sea level. The temperature of the lake is uniform with depth and identical to the air at the surface of the lake. To what depth should a balloon be taken under the lake to reduce its volume by a factor of 4? answer: 20m
Liquid nitrogen is often used as an effective coolant, as its boiling temperature is 77.0 K. A 0.750 kg block of iron with an initial temperature of 313.27 K is immersed in an insulated bath of liquid nitrogen with an initial temperature of 77.0 K. After the iron and the liquid nitrogen reach a state of thermal equilibrium, the iron block has cooled to a final a temperature of 77.0 K, and 198 g of liquid nitrogen has boiled off (vaporized). Assuming that the specific heat of iron over this temperature range is is 285 J/kg·K, What is the latent heat of vaporization of liquid nitrogen?
Assume Lake Michigan contains 4.90 x 1012 m³ of water, and assume the water's density is that of water at 20°C and 1 atm. (a) How much energy (in J) is required to raise the temperature of that volume of water from 12.2°C to 24.4°C? 4.1E19 From the density of water and the volume, what is the mass of the water? What is specific heat? How is it related to the energy input, mass, and temperature change? Use it to solve for the energy. Be careful with units. J (b) How many years would it take to supply this amount of energy by using a power of 1,400 MW generated by an electric power plant? 926 How is power related to energy and time? Knowing the energy from part (a), can you find the time? Be careful with units. Make sure you convert the time in seconds to years. yr
A cramming student warms 0.500 L of cold coffee in a Pyrex carafe. Full carafe of coffee at 20°F. How much coffee has spilled when the coffee and carafe reach 95°C? Given that the carafe is an isotropic solid, Pyrex has a linear thermal expansion coefficient of 3.3 x 10-6 K-1 and water (coffee) has 207 x 106 K-1.
A well-insulated aluminum calorimeter cup with mass of 231 g contains 271 g of liquid water at 25.1 °C. A 295-g silver figure of polar bear, with initial temperature of 96.5 °C, is dropped into the water. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/(kg · K), 910 J/(kg · K), and 4190 J/(kg · K). final temperature:
The "steam" above a freshly made cup of instant coffee is really water vapor droplets condensing after evaporating from the hot coffee. What is the final temperature of 205 g of hot coffee initially at 98.0°C if 3.18 g evaporates from it? The coffee is in a Styrofoam cup, and so other methods of heat transfer can be neglected. Assume that coffee has the same physical properties as water; its latent heat of vaporization is 539 kcal/kg and its specific heat is 1.00 kcal/(kg · °C).
A balloon filled with 3.50 kg of water at a temperature of 22°C is dropped from rest from an airplane. The airplane is 8000 m above the ground. There is air resistance acting on the balloon, and just before hitting the ground, the balloon is traveling at a speed of 200 m/s. For this problem, you can ignore the balloon material (its mass, specific heat etc…) and just treat the balloon as 3.50 kg of pure water. Also, assume g is a constant 9.8 m/s^2 during the entire fall and that the system of the water + surrounding air is a closed system. Assume that all internal energy change occurs in the water. a) Find the temperature of the water in the balloon just before hitting the ground. ( cm, water = 4186 J/kgK)
A small chunk of dry ice (solid carbon dioxide) at 195 K is added to a thermally insulatedcontainer filled with liquid nitrogen at its boiling point of 77 K. What happens in thecontainer?(A) The dry ice melts until thermal equilibrium is established.(B) Some of the liquid nitrogen boils and the dry ice gets colder.(C) Some of the liquid nitrogen freezes and the chunk of dry ice gets larger.(D) An equilibrium temperature is reached without any phase changes occurring.