   Chapter 17, Problem 9ALQ

Chapter
Section
Textbook Problem

# At 1 atm, liquid water is heated above 100°C. For this process, which of the following choices (i‒iv) is correct for ∆Ssurr? ∆S? ∆Suniv? Explain each answer.i. greater than zeroii. less than zeroiii. equal to zeroiv. cannot be determined

Interpretation Introduction

Interpretation: The correct choice, with respect to the given data, for ΔSsurr , ΔS and ΔSuniv is to be stated.

Concept introduction: The formula to calculate ΔSsurr is,

ΔSsurr=ΔHT

The formula to calculate ΔSuniv is,

ΔSuniv=ΔSsys+ΔSsurr

To determine: The correct choice, with respect to the given data, for ΔSsurr , ΔS and ΔSuniv .

Explanation

Explanation

(i)

Heat is being added to the given system. Water is converted from the liquid state to a gaseous state. Hence, the entropy value increases, that is, the entropy of the product is more than that of the reactant. Hence, the value of ΔS will be positive.

(ii)

The formula to calculate ΔSsurr is,

ΔSsurr=ΔHT

Where,

• ΔH is the change in enthalpy.
• T is the temperature.

The value of ΔH for an endothermic reaction is positive.

Therefore, for an endothermic reaction ΔSsurr will be unfavorable or negative (less than zero)

### 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 