Chapter 5, Problem 94IL

### 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 192-g piece of copper is heated to 100.0 °C in a boiling water bath and then dropped into a beaker containing 751 g of water (density = 1.00 g/cm3) at 4.0 °C. What was the final temperature of the copper and water after thermal equilibrium was reached? (CCu = 0.385 J/g · K.)

Interpretation Introduction

Interpretation:

At thermal equilibrium final temperature of copper and water has to be calculated.

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

Given values are:

Mass of the copper is 192â€‰g

Specific heat capacity of water is 0.385â€‰J/gK

Mass of water is 751â€‰g

Initial temperature of copper is 100â€‰0C

Initial temperature of copper is 4â€‰0C

Assume qmetalâ€‰=-â€‰qwater

Substitute values in q=CÃ—mÃ—Î”T

â€‚Â 192gâ€‰Ã—â€‰0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started