   Chapter 12, Problem 47P

Chapter
Section
Textbook Problem

A Styrofoam cup holding 125 g of hot water at 1.00 × 102°C cools to room temperature, 20.0°C. What is the change in entropy of the room? (Neglect the specific heat of the cup and any change in temperature of the room.)

To determine
The change in entropy of the room.

Explanation

Section1:

To determine: The thermal energy transferred to the room.

Answer: The thermal energy transferred to the room is 4.19×104J .

Explanation:

Given Info:

The temperature of hot water is 1.00×102°C .

Room temperature is 20°C .

Mass of water in the Styrofoam cup is 0.125kg

Formula to calculate the thermal energy transferred to the room is,

Q=mc|ΔT|

• m is the mass of water
• c is the specific heat capacity of water
• |ΔT| is the change in temperature

Since,

|ΔT|=1.00×102°C20°C=80°C

Substitute 0.125kg for m, 4186J/kg°C for c and 80°C for |ΔT| to find the thermal energy transferred,

Q=(0

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