A 1.27-kg sample of water at 14.5°C is in a calorimeter. You drop a piece of steel with a mass of 0.3 kg at 201°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation taken together don't affect the outcome, as we'll see later.Hint The final equilibrium temperature of water and steel is Incorrect°C.If the water is in a glass beaker with a mass of 0.22 kg, which in turn is in a calorimeter, with the beaker at the same temperature as the water, how will this affect the answer? Try answering before doing a detailed calculation. Final temperature will be lower but not significantly so.Final temperature will be significantly lower.Final temperature will be higher but not significantly so.Final temperature will be significantly higher.Correct Using the setup in (b), the final equilibrium temperature of water, glass beaker, and steel is Incorrect°C. A 1.27-kg sample of water at 14.5°C is in a calorimeter. You drop a piece of steel with a mass of 0.3 kg at201°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonableassumptions that any steam produced condenses into liquid water during the process of equilibration andthat the evaporation and condensation taken together don't affect the outcome, as we'll see later.Hinta. The final equilibrium temperature of water and steel is 18.803xC.b. If the water is in a glass beaker with a mass of 0.22 kg, which in turn is in a calorimeter, with thebeaker at the same temperature as the water, how will this affect the answer? Try answering beforedoing a detailed calculation.Final temperature will be lower but not significantly so.Final temperature will be significantly lower.O Final temperature will be higher but not significantly so.O Final temperature will be significantly higher.c. Using the setup in (b), the final equilibrium temperature of water, glass beaker, and steel isxc.X°C.18.793

Step 1 Let final temperature be T, then heat lost by steel is heat gained by water.…

Answered: A 1.27-kg sample of water at 14.5°C is…

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

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A 1.27-kg sample of water at 14.5°C is in a calorimeter. You drop a piece of steel with a mass of 0.3 kg at 201°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation taken together don't affect the outcome, as we'll see later.

Hint

The final equilibrium temperature of water and steel is Incorrect°C.
If the water is in a glass beaker with a mass of 0.22 kg, which in turn is in a calorimeter, with the beaker at the same temperature as the water, how will this affect the answer? Try answering before doing a detailed calculation.
- Final temperature will be lower but not significantly so.
- Final temperature will be significantly lower.
- Final temperature will be higher but not significantly so.
- Final temperature will be significantly higher.
Correct
Using the setup in (b), the final equilibrium temperature of water, glass beaker, and steel is Incorrect°C.

A 1.27-kg sample of water at 14.5°C is in a calorimeter. You drop a piece of steel with a mass of 0.3 kg at
201°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable
assumptions that any steam produced condenses into liquid water during the process of equilibration and
that the evaporation and condensation taken together don't affect the outcome, as we'll see later.
Hint
a. The final equilibrium temperature of water and steel is 18.803
xC.
b. If the water is in a glass beaker with a mass of 0.22 kg, which in turn is in a calorimeter, with the
beaker at the same temperature as the water, how will this affect the answer? Try answering before
doing a detailed calculation.
Final temperature will be lower but not significantly so.
Final temperature will be significantly lower.
O Final temperature will be higher but not significantly so.
O Final temperature will be significantly higher.
c. Using the setup in (b), the final equilibrium temperature of water, glass beaker, and steel is
xc.
X°C.
18.793

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