A vessel of water containing 300 kg of water is initially at 270 K. A 100 kg piece of metal, initially at 1300 K, is placed in the water vessel to cool and the vessel is closed. The specific heat of the metal is 0.6 kJ/kg K and 4.2 kJ/kg K for water. Assume the specific heats are constant and that the vessel is well insulated. a. Find the final equilibrium temperature after cooling. b. Find the amount of entropy generated within the vessel in kJ/K

A sample of water that is initially at 84.00C absorbs 500 kcal of heat. As a result, the liquid water becomes water vapor at 1150C. What is the mass of the water? (Some useful information: cwater = 1 cal/g0C, Lv,water = 540 cal/g, and csteam = 0.480 cal/g0 C.   a. 488 g   b. 788 g   c. 588 g   d. 888 g   e. 688 g

Question # 4  a) A rigid tank contains water vapor at 250 C and unknown pressure. When the tank is cooled to  124 C, the vapors start condensing. Find the initial pressure in the tank.  b) A piston–cylinder device initially contains 50 L of liquid water at 40°C and 200 kPa. Heat is  transferred to the water at constant pressure until the entire liquid is vaporized. i.What is the mass of the water?   ii.What is the final temperature?   iii. Determine the total enthalpy change.

A beaker of water sits in the sun until it reaches an equilibrium temperature of30°C. The beaker is made of 100 g of aluminum and contains 180 g of water. In an attempt to cool this system, a small block of ice at 0°C is added to the water.   a. Determine the exact mass of ice needed to melt (giving up its latent heat of fusion) and bring the water and beaker temperature down to 0°C. b. If the ice block has a mass of 100 g, determine the final temperature of the system. If it turns out that Tf = 0°C, determine how much ice remains unmelted.

A beaker of water sits in the sun until it reaches an equilibrium temperature of30°C.The beaker is made of 100 g of aluminum and contains 180 g of water. In an attempt to cool this system, a small block of ice at 0°C is added to the water. a. Determine the exact mass of ice needed to melt (giving up its latent heat of fusion) and bring the water and beaker temperature down to 0°C. b. If the ice block has a mass of 100 g, determine the final temperature of the system. If it turns out that Tf = 0°C, determine how much ice remains unmelted. c. Repeat your calculations for 50 g of ice.

need the correct ans

Solve the following problem and show your complete solutions for better understanding.

A rigid vessel of 0.5 m3 volume containing saturated steam at 109°C, how much heat must be removed to bring its temperature to 25°C. *

Sketch the process on the following state diagrams. For the purposes of your diagram(s), it may beuseful consider that increasing the magnetic field B at a fixed temperature would tend to increase the magnetization M, resulting in a more ordered material (i.e., lower entropy).

2. Two insulated cylinders A and B with volumes VA = 2.0 m³ and VB = 5.8 m³ contain chlorine gas at different pressures and temperatures. The cylinders are insulated (no heat is lost to or gained from the outside) and connected by a valve. Initially, the valve is) closed and the gas in the two cylinders has the following values: PA = 4.0x105 N/m², TA = 210 K, PB = 2.5x105 N/m², TB = 580 K. The valve is opened to allow the contents in the two cylinders to mix until the pressure equalizes. valve B a. Assuming there is no change in the temperatures of the containers themselves, determine the final temperature of the gas in the two cylinders. The atomic mass of chlorine gas is 35.4527 u. (1 u = 1.67377x1027 kg) b. Determine the final pressure?