Question

2.50 kg of water at 90 (degrees of C) is contained in a thermally-isolated container. A...

2.50 kg of water at 90 (degrees of C) is contained in a thermally-isolated container. A 1.50 kg chunk of ice at - 10 degrees C is added to the water, in the same thermally isolated container. a.) Describe the final state of the system when it has reached thermal equilibrium, give the final temperature and the amount of ice let (if any). b.) Find the net change in entropy of the system during this process.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 0.66300.6630 kg ice cube at −12.40−12.40 °C is placed inside a rigid, thermally isolated chamber...
A 0.66300.6630 kg ice cube at −12.40−12.40 °C is placed inside a rigid, thermally isolated chamber containing steam at 365.0365.0 °C. Later, you notice that the ice cube has completely melted into a puddle of water. The specific heats of ice, water, and steam are ?ice=2093 J/(kg·∘C),cice=2093 J/(kg·∘C), ?water=4186 J/(kg·∘C),cwater=4186 J/(kg·∘C), and ?steam=2009 J/(kg·∘C),csteam=2009 J/(kg·∘C), respectively. If the chamber initially contained 6.1906.190 moles of steam (water) molecules before the ice was added, calculate the final temperature ?fTf of the puddle...
Finding the equilibrium temperature of a mixture: An isolated thermal system consists of a copper container...
Finding the equilibrium temperature of a mixture: An isolated thermal system consists of a copper container filled with a quantity of liquid water and a quantity of ice. What is the fully thermalized state of the system (the final temperature, how much water, and how much ice) provided that initially there is 1.0 kg of ice at -100 degrees Celsius, 10 kg of water at 1 degrees Celsius, and the copper container has the mass of 15.0 kg and is...
23 g of water at 21°C is contained in a glass container of mass 327 g....
23 g of water at 21°C is contained in a glass container of mass 327 g. An additional 149 g of water at 100°C is added. What is the final equilibrium temperature (in degrees C) if we treat the system's water and container as isolated? Use the heat capacity values from the this table
20g of cream (3°C) is added to 200g of coffee (100°C) in a thermally isolated container.  If...
20g of cream (3°C) is added to 200g of coffee (100°C) in a thermally isolated container.  If both the coffee and cream have the specific heat of water (4186 J/kgK), what is the final temperature?
183 g of water at 21°C is contained in a copper container of mass 347 g....
183 g of water at 21°C is contained in a copper container of mass 347 g. An additional 124 g of water at 100°C is added. What is the final equilibrium temperature (in degrees C) if we treat the system's water and container as isolated? Use the heat capacity values from the this table. Specific heat capacity for copper is 387.
(a) Two 64 g ice cubes are dropped into 278 g of water in a thermally...
(a) Two 64 g ice cubes are dropped into 278 g of water in a thermally insulated container. If the water is initially at 25°C, and the ice comes directly from a freezer at −15°C, what is the final temperature at thermal equilibrium? (in celcius) (b) What is the final temperature if only one ice cube is used? (in celcius)
Finding the equilibrium temperature of a mixture: An isolated thermal system consists of a copper container...
Finding the equilibrium temperature of a mixture: An isolated thermal system consists of a copper container filled with a quantity of liquid water and a quantity of ice. What is the fully thermalized state of the system (the final temperature, how much water, and how much ice) provided that initially there is 1.0kg of ice at−100◦C, 10.0kg of water at 1◦C, and the copper container has the mass of 15.0kg and is initially at 10◦C? The heat capacities of ice,...
An insulated container has 2.00kg of water at 25◦C to which an unknown amount of ice...
An insulated container has 2.00kg of water at 25◦C to which an unknown amount of ice at 0◦C is added. The system comes to an equilibrium temperature of 20◦C. The heat capacity for water is 4190 J and the heat of fusion for ice is kg·K kJ LF =334kg. (a) Determine the amount of ice that was added to the water. (b) What is the change in the entropy associated with the ice melting? (c) What is the change in...
A perfectly insulated thermos contains 0.300 kg of water initially at 50 degrees C. A mass...
A perfectly insulated thermos contains 0.300 kg of water initially at 50 degrees C. A mass os of 0.100 kg of water initially at 10 degrees C is added. Ignore any heat exchanges with the outside environment. Take the specific heat capacity of liquid water as 4190 J/kgK. A) Draw a diagram for the situation, indicating the relative masses and temperatures. B) Find the final temperature of the combined water after they have mixed and attained thermal equilibrium (HINT: equate...
In a thermally isolated environment, you add ice at 0°C and steam at 100°C. (a) Determine...
In a thermally isolated environment, you add ice at 0°C and steam at 100°C. (a) Determine the amount of steam condensed (in g) and the final temperature (in °C) when the mass of ice and steam added are respectively 80.5 g and 10.9 g.(b) Repeat this calculation, when the mass of ice and steam added are interchanged. (Enter the amount of steam condensed in g and the final temperature in °C.) Very confused, Please explain