Chapter 5.2, Problem 5.2CYU

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# 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

Assume the sum of qwater+qchromium=0

The heat capacity of chromium can be calculated as,

â€‚Â CwaterÃ—Mwater(Tfinal-Tinitial)+CCrÃ—MCr(Tfinal-Tinitial)=0

Substitute for the above equation as

Specific heat capacity of water is 4

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