1. An insulated container contains 1.20kg of water with 0.73kg of ice floating in it. You place a...

1. An insulated container contains 1.20kg of water with 0.73kg of ice floating in it. You place a block of iron with mass of 4.60kg in this ice bath. The iron is initially at a temperature of 400 ºC. What is the composition and temperature of the final mixture?

For ice L_f=33.5x10⁴J/kg.

For water c=4186J/(kg•K).

For iron c=448 J/(kg•K).

2. A heat transfer of 9.5 x 10⁵ J is needed to convert a block of ice at -15°C to water at 15°C. What was the mass of the block of ice?

For ice L_f=33.5x10⁴J/kg.

For ice c=2090 J/(kg•K).

For water c=4186J/(kg•K).

Expert Solution

genius_generous answered 1 year ago

A 29.5g ice cube at -10 degrees celsius is place in a thermally insulated container along...

A 29.5g ice cube at -10 degrees celsius is place in a thermally insulated container along with 1.000kg of water initially at 20.0 degrees celsius. determine the final temperature of the system and the amount of heat acquired by the ice during the process and the amount of heat lost by the warm water. PLEASE SHOW WORK AND EQUATIONS USED. I'm struggling to find equations for heat gained, lost, and final temp. thank you.

What best describe ice floating in water?

A container contains water at 100 kPa. The specific volume of the water inside the container...

A container contains water at 100 kPa. The specific volume of the water inside the container is 1.00 m3/kg. What is the quality (x) of the water in the container, as a percentage and what is the phase of the water in the container?

An insulated container contains a gas with some initial conditions. A lid is opened which allows the gas to pass into another insulated container which was initially empty.

An insulated container contains a gas with some initial conditions. A lid is opened which allows the gas to pass into another insulated container which was initially empty. The mass of the gas remains constant. A process is described as reversible if there is no change in entropy. Explain in detail if this process is reversible or not.

An insulated container contains 15.0 g of steam at 100C. A mass of 65.0 g of...

An insulated container contains 15.0 g of steam at 100C. A mass of 65.0 g of ice at 0.00C is dropped into the container (assume no energy is absorbed by the container). C = Celsius a). How much heat is released by the steam when it condenses at 100C? (Qs) b). How much heat is absorbed by the ice when it melts at 0.00C? (Qi) c). What is the final temperature of the the water in the container? (T)

. Inside of a calorimeter (insulated container) is placed 200g of water at 20°C. The lid...

. Inside of a calorimeter (insulated container) is placed 200g of water at 20°C. The lid of the calorimeter is briefly lifted and 50g of lead is added initially at 200°C. What is the thermal equilibrium temperature? (3pts) 10. An object of mass 50kg is pushed in the +x direction with a force of 40N flat along a horizontal surface causing a net acceleration of 0.15m/s2 in the +x direction. What is the coefficient of kinetic friction between the surface...

A 65 g ice cube at 0 °C is placed in an insulated box that contains...

A 65 g ice cube at 0 °C is placed in an insulated box that contains 8 g of steam at 200 °C. What is the equilibrium temperature reached by this closed system? Approximate the specific heat capacity of steam to be 1.5 J/g oC. All the other values can be found on the textbook. [Note: Assume that all of the steam condenses.]

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0...

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5...

An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

3. An insulated container contains 2.7 kg of steam at 1.4 bar and 120°C. The top...

3. An insulated container contains 2.7 kg of steam at 1.4 bar and 120°C. The top is opened and a 1.8 kg block of ice at 0°C and 4.5 kg of liquid water at 1.6°C are dumped into the container. What is the final temperature of the resulting vapor-liquid mixture in the container? Note: It takes 6.0095 KJ/mol to melt ice.

Question