   # A 15.5-g piece of chromium, heated to 100.0 °C, is dropped into 55.5 g of water at 16.5 °C. The final temperature of the metal and the water is 18.9 °C. What is the specific heat capacity of chromium? (Assume no energy is lost to the container or to the surrounding air.) ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 5.2, Problem 2CYU
Textbook Problem
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## A 15.5-g piece of chromium, heated to 100.0 °C, is dropped into 55.5 g of water at 16.5 °C. The final temperature of the metal and the water is 18.9 °C. What is the specific heat capacity of chromium? (Assume no energy is lost to the container or to the surrounding air.)

Interpretation Introduction

Interpretation:

For a given mass of chromium placed in a beaker containing water the heat capacity of chromium has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1k.

Energy gained or lost can be calculated using the below equation.

q=C×m×ΔT

Where,

q= energy gained or lost for a given mass of substance (m)

C =specific heat capacity

ΔT = change in temperature.

### Explanation of Solution

Assume the sum of qwater+qchromium=0

The heat capacity of chromium can be calculated as,

Cwater×Mwater(Tfinal-Tinitial)+CCr×MCr(Tfinal-Tinitial)=0

Substitute for the above equation as

Specific heat capacity of water is 4

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