   # Chloroform is a common liquid used in the laboratory. It vaporizes readily. If the pressure of chloroform vapor in a flask is 195 mm Hg at 25.0 °C and the density of the vapor is 1.25 g/L, what is the molar mass of chloroform? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 26PS
Textbook Problem
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## Chloroform is a common liquid used in the laboratory. It vaporizes readily. If the pressure of chloroform vapor in a flask is 195 mm Hg at 25.0 °C and the density of the vapor is 1.25 g/L, what is the molar mass of chloroform?

Interpretation Introduction

Interpretation:

The molar mass of chloroform has to be determined.

Concept Introduction:

density=PMRT

P-PressureM-MolarmassR-UniversalgasconstantT-Temperature

### Explanation of Solution

Given that:

density=1.25g/LPressure=195mmHg=0.256atmTemperature=25°C=298K

Using this density we can calculate the molar mass of the compound.

density=PMRT

M=dRTP=1

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