Question

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

Homework Answers

Answer #1

final temperature is less than initial temperature of copper mean the energy going out of the copper is equal to the energy amount going into the aluminum. This means:

qlost = qgain

m1 * Cp1 * delta T = m2 * Cp2 * delta T

{ Cp of copper = 0.385 J/g.0C , Cp of aluminum = 0.902 J/g.0C }

So, by substitution, we then have:

(25.84 g) (97.16 0C - 53.87 0C) (0.385 J/g.0C) = (50.04 g) ( 53.87 0C - X) (0.902 J/g.0C)

Solve for X

430.66 = 2431.48 - 45.136 X

X = 44.329 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
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?
If 264.6 g sample of iron is placed in 1.005 L of water initially at 19.884oC...
If 264.6 g sample of iron is placed in 1.005 L of water initially at 19.884oC and both substances reach a final temperature of 28.151oC, what is the initial temperature (in oC) of the metal? Assume all heat is transferred between the water and the iron.
If 339.2 g sample of iron is placed in 1.025 L of water initially at 22.761oC...
If 339.2 g sample of iron is placed in 1.025 L of water initially at 22.761oC and both substances reach a final temperature of 27.488oC, what is the initial temperature (in oC) of the metal? Assume all heat is transferred between the water and the iron.  
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.
A 200 g of copper, initially at 300o C, is dropped into a 350 g of...
A 200 g of copper, initially at 300o C, is dropped into a 350 g of water contained in a 355 g aluminum calorimeter; the water and the calorimeter are initially 15o C. If 25 g iron stirrer is used to bring the mixture into thermal equilibrium, what is the final temperature of the system? ( Assume that the stirrer is initially at 15o C.) Specific heat of copper and aluminum are 0.092 cal/g oC and 0.215 cal/g oC respectively....
A sheet of aluminum weighing 100.0 g and at a temperature of 50.0 C is placed...
A sheet of aluminum weighing 100.0 g and at a temperature of 50.0 C is placed in contact with a piece of copper weighing 100.0 g and at a temperature of 100.0 C. 1) What do you expect to happen? Which metal is going to get warmer? Why? If you did not have a thermometer on the blocks, what visual cue would let you know one is hottter than the other? 2) Will the final temperature just be average of...
A hot lump of 26.3 g of aluminum at an initial temperature of 67.2 °C is...
A hot lump of 26.3 g of aluminum at an initial temperature of 67.2 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 46.2 g of copper at an initial temperature of 93.9 °C is...
A hot lump of 46.2 g of copper at an initial temperature of 93.9 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 27.5 g of copper at an initial temperature of 54.7 °C is...
A hot lump of 27.5 g of copper at an initial temperature of 54.7 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A 220-g sample of copper is heated to 100∘∘C and placed into a cup containing 320...
A 220-g sample of copper is heated to 100∘∘C and placed into a cup containing 320 g of water initially at 30.0∘∘C. Ignore the container holding the water, assume no heat is lost or gained to the environment. 1) Find the final equilibrium temperature of the copper and water.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT