Question

4. An iron container has a mass of 200 g and contains 50 g of water...

4. An iron container has a mass of 200 g and contains 50 g of water 40 C. 50 g of ice are poured at -6° C. Calculate the equilibrium temperature and describe the final composition.

5. We have a puddle of hot water @ 60 ° C exposed to air @ 28 ° C. Assume that the cooling constant of the water is 0.05/minutes. Calculate how long it will take the temperature on the surface of the water to go down to 42° C.

Homework Answers

Answer #1

4.

mi = mass of iron container = 200 g = 0.2 kg

mw = mass of water inside the container = 50 g = 0.050 kg

m = mass of ice poured = 50 g = 0.050 kg

To = initial temperature of iron container and water = 40 oC

Ti = initial temperature ice poured = - 6 oC

Tf = final equilibrium temperature = ?

ci = specific heat of iron = 0.450 J/gC

cw = specific heat of water = 4.2 J/gC

c = specific heat of ice = 2.11 J/gC

m' = mass of ice melted

using conservation of heat

heat lost by iron container + heat lost by water = heat gained by ice

mi ci (To - Tf ) + mw cw (To - Tf ) = m c (Tf - Ti) + m L

(0.2) (0.450) (40 - 0) + (0.050) (4.2) (40 - 0) = (0.050) (2.11) (0- (- 6)) + m' (334)

m' = 0.034 kg = 34 g

hence water = 34 + 50 = 84 g

ice = 50 g - 34 g = 16 g

final equilibrium temperature comes out to be 0 C since the heat of melting of the ice is greater than the heat lost by the iron container and water

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 student has a container that contains both 100.0 g of ice and 100.0 g of...
A student has a container that contains both 100.0 g of ice and 100.0 g of water that are coexisting at 0.0 C. Then the student adds 12 g of steam at 110 C to the mixture. What is the final temperature of this sytem? What is the final composition of the system? (How many grams of ice? Water? Steam?)
30.0-g of water is put into an iron container whose mass is 125 g. After the...
30.0-g of water is put into an iron container whose mass is 125 g. After the system comes into thermal equilibrium, only some of the water is evaporated. The amount of energy required to bring the water up to 100^o C is 370. cal. Once the water has reached 100^0 C, the amount of energy left (from the iron) to evaporate the water is 1,390 cal. What is the final equilibrium temperature of the system?
An iron calorimeter of mass 153 g contains 260 g of water. The system is in...
An iron calorimeter of mass 153 g contains 260 g of water. The system is in thermal equilibrium at +10°C. We place two blocks of metal in the water: one is a 45 g piece of copper with an initial temperature of +61°C; the second piece has a mass of 75 g and is initially at +100°C. The combined system reaches a final equilibrium temperature of +41°C. Calculate the specific heat capacity of the unknown second piece of metal.
A 500-g aluminum container holds 300 g of water. The water and aluminum are initially at...
A 500-g aluminum container holds 300 g of water. The water and aluminum are initially at 40∘C. A 200-g iron block at 0∘C is added to the water. Assume the specific heat of iron is 450 J/kg⋅∘C, the specific heat of water 4180 J/kg⋅∘C and the specific heat of aluminum is 900 J/kg⋅∘C . 1Determine the final equilibrium temperature.    2.Determine the change in thermal energy of the aluminum 3.Determine the change in thermal energy of the water. 4. Determine...
A thermally insolated vessel contains 250 g of water and 100 g of ice in thermal...
A thermally insolated vessel contains 250 g of water and 100 g of ice in thermal equilibrium at normal pressure. Then, a certain amount of hot steam at 140 oC is added. After waiting for a long enough time, the temperature inside the vessel is settled at 50 oC. How much steam was injected?
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 sphere of iron is heated up to 1000° C. Once heated, it has a radius...
A sphere of iron is heated up to 1000° C. Once heated, it has a radius of 1 cm. Now suppose that we take the same 1000° C iron sphere and plunge it into a thermally insulated container with 1kg of 0° C ice. Calculate the temperature of the contents of the container once they have come to thermal equilibrium. Additional information: • The density of iron is 7.874 g/cm3. Assume that this density does not depend on temperature. •...
A few iron nails with a total mass of 22.4 g are heated in a water...
A few iron nails with a total mass of 22.4 g are heated in a water bath for five minutes. The water bath was boiling with a constant temperature of 101°C according to the thermometer. When the nails were carefully transferred into 182.0 g of water in a coffee cup calorimeter the temperature of the water rose from 25.0°C to 26.0°C. What is the heat capacity of the iron?
An 890-g iron block is heated to 370 ∘C and placed in an insulated container (of...
An 890-g iron block is heated to 370 ∘C and placed in an insulated container (of negligible heat capacity) containing 35.0 g of water at 20.0 ∘C. What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg⋅K). Answer in ∘C. I have already tried 109 ∘C and 110 ∘C, so I don't know what I'm doing wrong. :(
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT