Chapter 11, Problem 12PS

### 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

# The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.500 mL of mercury at 357 °C, its normal boiling point? The density of mercury is 13.6 g/mL.

Interpretation Introduction

Interpretation: The energy required to evaporate the given volume of mercury has to be determined.

Concept Introduction:

The energy required to overcome the intermolecular forces of attraction for 1mol of a substance is called standard enthalpy of vaporization,ΔvapH0

Equation for density is,

Density=MassVolume

From its given mass is,

Number of moles=GivenmassMolecularmass

Explanation

Given,

Densityâ€‰=â€‰13.6g/mLâ€‰Volumeâ€‰=â€‰0.500mLMolarâ€‰massâ€‰=â€‰200.59â€‰g/molEnthaplyâ€‰ofâ€‰vaporization,Î”vapH0â€‰=â€‰59.11â€‰kJ/mol

Equation for density is,

â€‚Â Densityâ€‰â€‰=â€‰â€‰â€‰MassVolumeâ€‰

Hence,

The mass of ethanol is,

â€‚Â Massâ€‰=â€‰DensityÃ—â€‰Volume=â€‰(13.6g1mL)â€‰Ã—â€‰0.500â€‰mL=â€‰6.8â€‰g =2

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