Question

A 116 g insulated aluminum cup at 15

A 116 g insulated aluminum cup at 15

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

We need to find the final temperature of the system. Assuming no losses, the cup and water will end up at the final temperature T?

Specific Heat from link
C_aluminum = 0.215
C_water = 1.00

Q_cup + Q_water = 0
M_cup C_cup ?T_cup + M_water C_water ?T_water = 0
116g * 0.215 * ?T_cup + 140g * 1 * ?T_water = 0
24.94 ?T_cup + 140 ?T_water = 0
24.94 (T? - T?_cup) + 140 (T? - T?_water) = 0
24.94 T? - 24.94 T?_cup + 140 T? - 140 T?_water = 0
164.94 T? = 24.94 T?_cup + 140 T?_water

T? = (24.94 T?_cup + 140 T?_water)/164.94
= (24.94 * 15

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
You drop a 291-g silver figure of a polar bear into the 247-g aluminum cup of...
You drop a 291-g silver figure of a polar bear into the 247-g aluminum cup of a well-insulated calorimeter containing 261 g of liquid water at 21.9°C. The bear\'s initial temperature is 97.9°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and 4190 J/(kg·K).
You drop a 297-g silver figure of a polar bear into the 247-g aluminum cup of...
You drop a 297-g silver figure of a polar bear into the 247-g aluminum cup of a well-insulated calorimeter containing 259 g of liquid water at 22.3°C. The bear\'s initial temperature is 98.5°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and 4190 J/(kg·K).
You drop a 285-g silver figure of a polar bear into the 241-g aluminum cup of...
You drop a 285-g silver figure of a polar bear into the 241-g aluminum cup of a well-insulated calorimeter containing 263 g of liquid water at 23.9°C. The bear\'s initial temperature is 95.9°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and 4190 J/(kg·K).
You drop a 297-g silver figure of a polar bear into the 205-g aluminum cup of...
You drop a 297-g silver figure of a polar bear into the 205-g aluminum cup of a well-insulated calorimeter containing 277 g of liquid water at 24.5°C. The bear\'s initial temperature is 95.5°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and 4190 J/(kg·K).
157 grams of aluminum at 367 degrees Kelvin is placed in a well insulated cup with...
157 grams of aluminum at 367 degrees Kelvin is placed in a well insulated cup with 2.3 kilograms of water at 299 degrees Kelvin. What is the increase in the system's entropy (in J/K) by the time it reaches equilibrium temperature? The specific heat capacity of water is 4200 J/Kg/K and of the aluminum is 900 J/Kg/K.
The aluminum cup inside your calorimeter weighs 40.85 g. You add 49.81 g of water and...
The aluminum cup inside your calorimeter weighs 40.85 g. You add 49.81 g of water and 3.03 g of KCl to the calorimeter. The initial temperature is 20.1oC, and the final temperature is 16.9oC. What is the heat of dissolution for the amounts of salt added, in units of J? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup. the mass of KCl added is small enough...
An aluminum cup contains 225 g of water and a 40 g copper stirrer, all at...
An aluminum cup contains 225 g of water and a 40 g copper stirrer, all at 27°C. A 470 g sample of silver at an initial temperature of 89°C is placed in the water. The stirrer is used to stir the mixture gently until it reaches its final equilibrium temperature of 32°C. Calculate the mass of the aluminum cup.
The aluminum cup inside your calorimeter weighs 39.96 g. You add 49.96 g of ice cold...
The aluminum cup inside your calorimeter weighs 39.96 g. You add 49.96 g of ice cold water to the calorimeter. You measure the temperature of the calorimeter to be 0.5oC just before your next addition. You then add 50.44 g of hot water and a 50.10 g metal object, all having an initial temperature of 69.5oC. After the calorimeter reaches thermal equilibrium, the final temperature is measured to be 36.1oC. Assume that: the calorimeter is completely insulated the heat capacity...
A 26.5 −g aluminum block is warmed to 65.4 ∘C and plunged into an insulated beaker...
A 26.5 −g aluminum block is warmed to 65.4 ∘C and plunged into an insulated beaker containing 55.1 g water initially at 22.2 ∘C. The aluminum and the water are allowed to come to thermal equilibrium.
A 27.0 −g aluminum block is warmed to 65.6 ∘C and plunged into an insulated beaker...
A 27.0 −g aluminum block is warmed to 65.6 ∘C and plunged into an insulated beaker containing 55.1 g water initially at 22.4 ∘C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT