Chapter 6, Problem 6.51P

There is an 500g container made out of aluminum holding 300g of water. The Water and Aluminum have reached thermal equilibrium at 40 degrees Celsius. A 200g block of iron at a temperature of 0 degrees Celsius is later dropped into the water. Using the specific heat for water=4180J/kg/C. The specific heat for aluminum is 900 J/kg/C. The specific heat for iron is 450 J/kg/C. The final temperature of the three materials will be degrees celsius. The thermal energy of the water changes by Joules. (give an amount and include a + if it increases and a - if it decreases) The thermal energy of the aluminum changes by Joules. (give an amount and include a + if it increases and a - if it decreases) The thermal energy of the iron changes by Joules. (give an amount and unit and include a + if it increases and a - if the value decreases)

According to the thermodynamic data below for a hypothetical single-component system, what is the approximate melting temperature of this system if it is heated slowly such that equilibrium conditions are met? G L 8 Y B a 0 100 200 300 400 L 500 8678 a 600

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A 390-g metal container, insulated on the outside, holds 170.0 g of water in thermal equilibrium at 21.0°C. A 18.0-g ice cube, at -15.0°C, is dropped into the water, and when thermal equilibrium is reached the temperature is 12.0°C. Assume there is no heat exchange with the surroundings. The specific heat capacity of water is 4190 J/kg ∙ K, the specific heat capacity of ice is 2090  J/kg ∙ K and the heat of fusion is 3.34 × 105 J/kg. What is the specific heat capacity of the metal of the container?

WA 4. a Th To Room temperature T = 293 K %3D V The gas volume changes from Vp to Va at constant temperature T. The cartoon on the right shows a piston of gas undergoing this compression while submerged in a container of room temperature water, which acts as a reservoir. The initial state of this process is a piston containing 2 moles of a monatomic gas at T, = 293 K (room temperature water) and volume V = 1.0 m. The gas is compressed until V, = 0.2 m. During the compression, the heat bath of room temperature water maintains the temperature of the gas at T = 293 K. Calculate the change in internal energy of the gas in joules during this process. Do not include units in your answer. Be careful to use the standard sign conventions for heat and work. Write your numerical answer in normal form as described above in the instructions to this worksheet. Click Save and Submit to save and submit. Click Save All Answers to save all answers. 28 F a

A mass of 12 kg of Oxygen occupying 3 m3 is heated from 25°C at a constant volume. Take gas constant is 0.297 kJ/kgK, then its initial pressure would be approximately 0.78 bar. Select one: O True O False

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A 50-kg iron block at 80°C is dropped into an insulated tank that contains 500 kg of liquid water at 25°C. Determine the final temperature when the thermal equilibrium is reached, in °C. (Specific. heat of water = 4.18 kJ/kg.°C) 55.2 25.6 24.8

The initial state of 1.00 mol of a dilute gas is P1 = 3.00 atm, V1 = 1.00 L, and Eint 1 = 456 J and its final state is P2 = 2.00 atm, V2 = 3.00 L, and Eint2 = 912 J. The gas is first cooled at constant volume until it reaches its final pressure. It is then allowed to expand at constant pressure until it reaches its final volume. (a) Illustrate this process on a PV diagram and calculate the work done by the gas. (b) Find the heat absorbed by the gas during this process.