Question

In: Physics

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water...

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water at 100 ∘C

a) Determine the final temperature of the mixture.

b)  Determine the total change in entropy as a result of the mixing process (use ΔS=∫dQ/T).

Solutions

Expert Solution

Solution :-

  1. Find final temperature

Assumeing no losses the cup and water will end up at the final temp T2.

Specific heat from link

C aluminium – 0.215

C water – 1.00

Q cup + Q Water = 0

M cup C cup ΔT – cup + M water c water ΔT water = 0

200g * 0.215 * ΔT cup + 200g * 1 * ΔT water = 0

  1. ΔT cup + 255 ΔT water = 0

43( T2 – T1 cup) + 255 (T2 – T1Water ) = 0

43T2 – 43T1 cup + 255T2 –T1 water = 0

298T2 = 43T1cup + 255T1 water

T2 = ( 43T1 cup + 255 T2 water ) / 298

T2 = (43*160C + 255 * 1000C ) / 298

T2 = 688 + 25500 / 298

T2 = 87.80C

The final temperature is = T2 = 87.80C

       b ) Determine total change in enyropy

  1. 160C - 273 + 16 = 289 K
  2. 87.80C = 87.8 + 273 360.8 K
  3. 1000C = 100 + 373 = 293K

Using formula ΔS = Dq / T

  • S = ΔS * Cup + ΔS water
  • S= Q cup / T aver + Q water / Tave

(MCΔT)-cupT ave + (MCΔT)-water /T ave

( 200*0.215*(360.8 – 289 ) /*(360.8 + 289 )/ 2

( 2555*1*(360.8 – 373 ) /*(360.8 +373 )/ 2 /2

30616 / 324.6 + 3111 / 366.9

9.4319162 – 8.4791

= 0.952

= ΔS

total change in entropy - 0.952

  


Related Solutions

28 g of ice at -10⁰C is dropped in an insulated 75-g aluminum calorimeter cup containing...
28 g of ice at -10⁰C is dropped in an insulated 75-g aluminum calorimeter cup containing 140 g of water at 30⁰C. (a) Calculate the equilibrium temperature of the container. Specific heats of liquid water, ice and aluminum are 4186 J/(kg ⁰C), 2090 J/(kg ⁰C) and 910 J/(kg ⁰C)respectively. Latent heat of fusion for ice is 3.33 x 105 J/kg. (b) What if, find the final temperature if 68 g of ice had been dropped.
28 g of ice at -100C is dropped in an insulated 75-g aluminum calorimeter cup containing...
28 g of ice at -100C is dropped in an insulated 75-g aluminum calorimeter cup containing 140 g of water at 300C. (a) Calculate the equilibrium temperature of the container. Specific heats of liquid water, ice and aluminum are 4186 J/(kg 0C), 2090 J/(kg 0C) and 910 J/(kg 0C)respectively. Latent heat of fusion for ice is 3.33 x 105 J/kg. (b) What if, find the final temperature if 68 g of ice had been dropped.
A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g...
A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. Find the final temperature of the system, assuming no heat losses. (The specific heat of ice is 2.0 kJ/kg K) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? Would your answer to part b be different if...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. A) Find the final temperature of the system, assuming no heat losses. (Assume that the specific heat of ice is 2.0 kJ/kg K) B) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? C) Would your answer...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. Find the final temperature of the system, assuming no heat losses. (Assume that the specific heat of ice is 2.0 kJ/kg K) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? Would your answer to part b...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of water at 25.0°C. Determine the amount of steam (in g) needed for the system to reach a final temperature of 64.0°C. The specific heat of aluminum is 900 J/(kg · °C).
A 26.0-g aluminum block is warmed to 65.1 ∘C and plunged into an insulated beaker containing...
A 26.0-g aluminum block is warmed to 65.1 ∘C and plunged into an insulated beaker containing 55.5 g of water initially at 22.3 ∘C . The aluminum and the water are allowed to come to thermal equilibrium. (Cs,H2O=4.18J/g⋅∘C , Cs,Al=0.903J/g⋅∘C ) Assuming that no heat is lost, what is the final temperature of the water and aluminum? T = ??      ∘C     
1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial...
1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial temperature is 70?C. The system comes to an equilibrium temperature of 20?C. What is the mass of the cup in kg. 2.Radiation from the head is a major source of heat loss from the human body. Model a head as a 20-cm-diameter, 20-cm-tall cylinder with a flat top.If the body's surface temperature is 36 ?C , what is the net rate of heat loss...
A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g...
A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g piece of ice is cooled to −20.0 °C and then placed in the calorimeter. Use the following specific heats: cAl = 900.0 J Kg-1 °C-1, cwater = 4186 J Kg-1 °C-1, cice = 2.10 x 103 J Kg-1 °C-1. The latent heat of fusion for water is LF = 333.5 x 103 J/Kg. (a) Find the final temperature of the system, assuming no heat...
A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C . A 124.0-g block of...
A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C . A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g⋅K . The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.3 ∘C . Part A Determine the amount of heat, in J , lost by the copper block....
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT