Question

A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC....

A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC. The calorimeter contains 42.3 g of deoinized water. The initial temperature of the water is 22.3 oC. The metal is transferred to the calorimeter and the final temperature reached by the water + metal is 32.2 oC.

A. Calculate ∆T for the water (Tfinal – Tinitial).

B. Calculate ∆T for the metal.

C. The specific heat of water is 4.18 J/goC. Calculate the specific heat of the metal.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in...
3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in a calorimeter containing 50 g of water at 25.0 oC. At equilibrium the temperature of water and metal was 35.5 oC. Calculate the heat capacity of the metal. . Use this value for Cp:27.65. 4. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 oC to...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling...
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 47.5 block of an unknown metal is heated in a hot water bath to 100...
A 47.5 block of an unknown metal is heated in a hot water bath to 100 degrees Celsius. When the block is placed in an insulated vessel containing 130.0 g of water at 25.0 degrees Celsius, the final temperature is 28.0 degrees Celsius. Determine the specific heat of the unknown metal. The Cs for water is 4.18 J/g degrees Celsius.
1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water...
1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 27.0°C. - How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) - What is the specific heat (in J/g·°C) of the metal? 2. A 0.529 g sample of KCl is added...
A coin with a mass of 39.0 g is in a hot‐water bath at 97.00°C. A...
A coin with a mass of 39.0 g is in a hot‐water bath at 97.00°C. A calorimeter contains 175 g of water at 10.00°C. The hot coin is quickly moved and immersed in the cool water in the calorimeter. After stirring, the water and coin reach a final temperature of 12.00°C. Calculate the specific heat of the coin in J/(g x degree C) a. 0.473 b. 0.387 c. 0.540 d. 0.219 e. 0.442
PART A) A sample of metal at a known hot temperature is placed in to a...
PART A) A sample of metal at a known hot temperature is placed in to a calorimeter containing water of known mass and known initial temperature. The temperature of the water rises and the final temperature of the water is recorded. What equation is used to calculate the amount of heat the calorimeter water absorbed? PART B) How do you deermine the amount of heat lost by the metal if you know the amount of heat gained by the calorimeter...
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.
1.) A volume of 36.7 mL of H2O is initially at 28.0 oC. A chilled glass...
1.) A volume of 36.7 mL of H2O is initially at 28.0 oC. A chilled glass marble weighing 4.00 g with a heat capacity of 3.52 J/oC is placed in the water. If the final temperature of the system is 26.4  oC , what was the initial temperature of the marble? Water has a density of 1.00 g/mL and a specific heat of 4.18 J/goC. Enter your answer numerically, to three significant figures and in terms of oC. 2.) A 2.24...
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:...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT