Thermodynamics: Dropping a hot horseshoe into a pot of water

In summary, the mass of the horseshoe, pot, and water were provided, along with their initial and final temperatures. The amount of heat gained by the pot and water as they cool the horseshoe was calculated to be 57241.38 J, which is not rounded to 3 significant figures.
  • #1
Jess_18033152
32
0

Homework Statement


A freshly-forged iron horseshoe, with a mass of 0.549 kg is dropped into a 0.281 kg iron pot which contains 1.60 kg of water at 21.4 oC.
After the horseshoe, pot and water reach thermal equilibrium they have a temperature of 29.8 oC.

Assuming the pot and the water were in thermal equilibrium before the horseshoe entered the water, calculate the combined amount of heat gained by the pot and water as they cool the horseshoe.

From previous question:
Initial temp of horseshoe = 261.499575 degrees C
Q (water) = 56179.2 J
Q (pot) = 1062.18 J

Homework Equations


Q= mc (change in temp)

The Attempt at a Solution


Q (horseshoe) = 0.549 x 450 x (261.499575-29.8)
= 57241.38 J

Q (water) = 56179.2 J
Q (pot) = 1062.18 J
Q (pot & water) = 56179.2 + 1062.18
= 57241.38 J

Am I heading in the right direction to calculate the combined amount of heat gained by the pot and water as they cool the horseshoe?
 
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  • #2
Worked out that the answer for this question is just = 57241.38 J rounded to 3 significant figures. :)
 
  • #3
Jess_18033152 said:
Worked out that the answer for this question is just = 57241.38 J rounded to 3 significant figures. :)
Do you really feel that that is rounded to 3 significant figures?
 
  • #4
Sorry, that my answer from that I rounded to 3 sf so that wasn't my final answer as it is not 3 sf
 

What is thermodynamics?

Thermodynamics is the study of energy and its transformation from one form to another.

What happens when a hot horseshoe is dropped into a pot of water?

When a hot horseshoe is dropped into a pot of water, the energy from the horseshoe is transferred to the water, causing it to heat up.

What is the significance of this experiment?

This experiment demonstrates the principles of heat transfer and the laws of thermodynamics.

What are the three laws of thermodynamics?

The first law states that energy cannot be created or destroyed, only transferred or converted. The second law states that in any energy transfer or conversion, some energy will always be lost as heat. The third law states that at absolute zero temperature, the entropy of a pure, perfect crystalline substance is zero.

What are some real-life applications of thermodynamics?

Thermodynamics is used in many fields, including engineering, chemistry, and biology. It is essential for understanding and designing systems such as power plants, refrigeration systems, and chemical reactions. It also plays a crucial role in understanding biological processes and ecosystems.

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