Question

50 g Cu (c=24.5J/K/mol) is heated to 100C and then placed in 250g water(c=4.184J/g/K) at 0C....

50 g Cu (c=24.5J/K/mol) is heated to 100C and then placed in 250g water(c=4.184J/g/K) at 0C. What is the final temperature of water (in C)?

Homework Answers

Answer #1

we know that the heat gained by water will be the heat lost by the metal.

The heat lost by metal = mole of metal X heat capacity of metal X change in temperature

Mass of copper = 50g

Atomi weight = 63.5

So moles = Mass ./ atomic weight = 50 / 63.5 = 0.79

Heat lost by metal = 0.79 X 24.5 X (final temperarure - 100)

Heat gained by water = mass of water X heat capacity of water X change in temperature

Heat gained by water = 250 X 4.184 X (final temperatre - intial temperature) = 250 X 4.184 X (final temperature - 0)

0.79 X 24.5 X (T2-100) = 250 X 4.184 X (T2-0)

1936 - 19.36 X T2 = 1046 T2

890 = 19.36T2

T2 = 45.97

so the final temperature = 45.97 0C

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
150 g of ice at 0C is placed into 100 g of water at 15C. What...
150 g of ice at 0C is placed into 100 g of water at 15C. What is the final temperature of the system and how much ice is left at the end?
A 53.0-g metal weight, heated to 87.50°C, is placed into 191 g of water at 21.05°C...
A 53.0-g metal weight, heated to 87.50°C, is placed into 191 g of water at 21.05°C contained in a perfectly insulating thermos flask. After some time, the temperature inside the thermos flask stabilizes at 23.80°C. The specific heat capacity of water is approximately 4.18 J/K/g in the temperature range 16°C - 61°C. Calculate the specific heat capacity of the metal.
2. A 35g ball of brass at 25 0C is placed in a pot of boiling...
2. A 35g ball of brass at 25 0C is placed in a pot of boiling water reading 120 0C until equilibrium is reached. How much thermal energy is absorbed by the ball?[ specific heat of brass = 393.5 J/Kg 0C] a. 1.3 mJ b. 1.3 MJ c. 1.3 kJ d. 1.3 J 2. A 40-g mass of an unknown material at 90 0C is placed in 250 g of water at an initial temperature of 15.0 0C. The final...
. A bag of ice containing 325 g of ice at 0 0C was placed on...
. A bag of ice containing 325 g of ice at 0 0C was placed on a patient’s sore thigh muscles. When the ice bag was removed, all the ice had melted, and the liquid water in the bag had a temperature of 18 0C. (a) What was the final volume of liquid water in the ice bag?
1- The molar mass and molar heat capacity of aluminum is 27.0 g/mol and 24.3 J/(mol...
1- The molar mass and molar heat capacity of aluminum is 27.0 g/mol and 24.3 J/(mol K), respectively. If a 27.0-g Al sample, at 300. K, absorbed 168 J of heat, what is its final temperature? 2- The molar mass and molar heat capacity of aluminum is 27.0 g/mol and 24.3 J/(mol K), respectively. If a 27.0-g Al sample, at 300. K, absorbed 152 J of heat, what is its final temperature? 3- 100. g water, at 20 C, and...
A 48.2 g sample of a metal is heated to 95.8 degrees C and placed in...
A 48.2 g sample of a metal is heated to 95.8 degrees C and placed in a coffee-cup calorimeter containing 79.0 g of water at a temperature of 18.5 degrees C. After the metal cools, the final temperature of the metal and water is 22.8 degrees C. Calculate the specific heat capacity of the metal, assuming that no heat escapes to the surroundings or is transferred to the calorimeter.
Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water at 25.0...
Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H2O(s) is 37.7 J/mol*K heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20 is 6.01 kJ/mol
Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water at 25.0...
Two 20.0-g ice cubes at –13.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of H2O(s) 37.7 J/(mol*k) heat capacity of H2O(l) 75.3 J/(mol*k) enthalpy of fusion of H2O 6.01 kJ/mol
A 401−g piece of copper tubing is heated to 89.5°C and placed in an insulated vessel...
A 401−g piece of copper tubing is heated to 89.5°C and placed in an insulated vessel containing 159 g of water at 22.8°C. Assuming no loss of water and a heat capacity for the vessel of 10.0 J/°C, what is the final temperature of the system (c of copper = 0.387 J/g·°C)?
A 404−g piece of copper tubing is heated to 89.5°C and placed in an insulated vessel...
A 404−g piece of copper tubing is heated to 89.5°C and placed in an insulated vessel containing 159 g of water at 22.8°C. Assuming no loss of water and a heat capacity for the vessel of 10.0 J/°C, what is the final temperature of the system (c of copper = 0.387 J/g·°C)?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT