   Chapter 10, Problem 28PS

Chapter
Section
Textbook Problem

A 0.0130-g sample of a gas with an empirical formula of C4H5 is placed in a 165-mL flask. It has a pressure of 13.7 mm Hg at 22.5 °C. What is the molecular formula of the compound?

Interpretation Introduction

Interpretation:

The molecular formula of the compound has to be determined.

Concept Introduction:

density=PMRT

P-PressureM-MolarmassR-UniversalgasconstantT-Temperature

Explanation

Given that:

massofthecompound=0.0130gvolume=165ml=0.165LPressure=13.7mmHg=0.018atmTemperature=22.5°C=295.5K

The molecular formula of the given gas can be calculated as

density=massvolume=0.0130g0.165L=0.07878g/L

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

density=PMRT

M=dRTP=0

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