Question

256 g of aluminum at 212.5 oC are placed in an insulated container with 22.2 g...

256 g of aluminum at 212.5 oC are placed in an insulated container with 22.2 g of mercury at 13.8 oC. What is the final temperature for the two metals in the container? (The specific heat of mercury is 0.139 J/g oC.

Homework Answers

Answer #1

m(mercury) = 22.2 g

T(mercury) = 13.8 oC

C(mercury) = 0.139 J/goC

m(aluminium) = 256.0 g

T(aluminium) = 212.5 oC

C(aluminium) = 0.902 J/goC

T = to be calculated

Let the final temperature be T oC

use:

heat lost by aluminium = heat gained by mercury

m(aluminium)*C(aluminium)*(T(aluminium)-T) = m(mercury)*C(mercury)*(T-T(mercury))

256.0*0.902*(212.5-T) = 22.2*0.139*(T-13.8)

230.912*(212.5-T) = 3.0858*(T-13.8)

49068.8 - 230.912*T = 3.0858*T - 42.584

T= 210. oC

Answer: 210. oC

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
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially...
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially at 111.86oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 36.38oC, what is the inital temperature (in oC) of aluminum?
An 50.04 g sample of aluminum is placed on a 25.84 g sample of copper initially...
An 50.04 g sample of aluminum is placed on a 25.84 g sample of copper initially at 97.16oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 53.87oC, what is the inital temperature (in oC) of aluminum
A (18) g ice cube at –15.0°C is placed in (126) g of water at 48.0...
A (18) g ice cube at –15.0°C is placed in (126) g of water at 48.0 degreesC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in degreesC with 3 significant figures. Specific heat of ice: 2.090 J/(g∙ oC) Specific heat of water: 4.186 J/(g∙ oC) Latent heat of fusion for water:...
What is the final temperature (in oC) of a 38 g sample of aluminum (specific heat...
What is the final temperature (in oC) of a 38 g sample of aluminum (specific heat = 0.900 J/(g K)) which absorbs 89.9 kJ of heat when it warms from 74.6oC?
A 26.5-g aluminum block is warmed to 65.2 ∘Cand plunged into an insulated beaker containing 55.2...
A 26.5-g aluminum block is warmed to 65.2 ∘Cand plunged into an insulated beaker containing 55.2 g of water initially at 22.2 ∘C. The aluminum and the water are allowed to come to thermal equilibrium. (Cs,H2O=4.18 J/g⋅∘C, Cs,Al=0.903J/g⋅∘C)​ Assuming that no heat is lost, what is the final temperature of the water and aluminum?​
A 25 g ice cube at -15.0oC is placed in 169 g of water at 48.0oC....
A 25 g ice cube at -15.0oC is placed in 169 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...
A 16 g ice cube at -15.0oC is placed in 140 g of water at 48.0oC....
A 16 g ice cube at -15.0oC is placed in 140 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...
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. :(
A 60.0 g aluminum block, initially at 55.00 °C, is submerged into an unknown mass of...
A 60.0 g aluminum block, initially at 55.00 °C, is submerged into an unknown mass of water at 293.15 K in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 25.00 °C. What is the approximate mass of the water? The specific heat of water is 4.18 J/g . °C. The specific heat of aluminum is 0.897 J/g . °C.
A (10.0+A) g ice cube at -15.0oC is placed in (125+B) g of water at 48.0oC....
A (10.0+A) g ice cube at -15.0oC is placed in (125+B) g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...