   Chapter 10.5, Problem 10.3SC ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
22 views

# ercise 10.3 A 5.63-g sample of solid gold is heated from 21 to 32 °C. How much energy (in joules and calories) is required?

Interpretation Introduction

Interpretation:

The amount of energy in joules and calories should be calculated when 5.63 g sample of gold is heated from 21 °C to 32 °C.

Concept Introduction:

Thus, formula used for calculate energy in joules is E=mcΔT

Where, E = energy in joules

m = mass of gold

c = specific heat capacity of gold

ΔT = change in temperature

A conversion factor is a numerical ratio which is used to show a measurement in one unit as another unit. It is always equal to 1.

Explanation

Specific heat capacity of gold is 0.13 Jg°C, as it takes, 0.13 J of energy to change the temperature of each gram of gold by 1 °C.

Therefore, multiply 0.13 J by the mass of water and temperature change.

ΔT (Temperature change) = 32°C21°C = 11 °C.

So,

Energy in joules = 0.13 Jg°C×5.63 g×11°C

= 8

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