Chapter 5, Problem 76GQ

### 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

# Calculate the quantity of energy required to convert 60.1 g of H2O(s) at 0.0 °C to H2O(g) at 100.0 °C. The enthalpy of fusion of ice at 0 °C is 333 J/g; the enthalpy of vaporization of liquid water at 100 °C is 2256 J/g.

Interpretation Introduction

Interpretation:

The quantity of heat required to convert a definite mass of H2O(s) 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.

The heat of the substance can be calculated as:

q=heat of fusion or vaporization × mass

Explanation

To melt at 00C

The mass of the H2O is 60.1g

The heat of fusion of ice is 333J/g

â€‚Â q=heat of fusion Ã— mass of H2O

â€‚Â q1=60.1gÃ—333J/g=2.0Ã—104J

To raise the temperature from 00C to 1000C

The mass of the water is 4.184â€‰J/gK

Mass of the water is 60.1â€‰g

The change in temperature is 100â€‰K

â€‚Â q2=4.184J/gKÃ—60.1gÃ—100K=2.5Ã—104J

To evaporate at 1000C

The mass of the H2O is 60

### 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