   # A new boron hydride, B x H y , has been isolated. To find its molar mass, you measure the pressure of the gas in a known volume at a known temperature. The following experimental data are collected: Mass of gas = 12.5 mg Pressure of gas = 24.8 mm Hg Temperature = 25 ° C Volume of flask = 125 mL Which formula corresponds to the calculated molar mass? (a) B 2 H 6 (b) B 4 H 10 (c) B 5 H 9 (d) B 6 H 10 (e) B l0 H 14 ### 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 29PS
Textbook Problem
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## A new boron hydride, BxHy, has been isolated. To find its molar mass, you measure the pressure of the gas in a known volume at a known temperature. The following experimental data are collected:Mass of gas = 12.5 mg Pressure of gas = 24.8 mm HgTemperature = 25 °C Volume of flask = 125 mLWhich formula corresponds to the calculated molar mass? (a) B2H6 (b) B4H10 (c) B5H9 (d) B6H10 (e) Bl0H14

Interpretation Introduction

Interpretation:

The molecular formula that corresponds to the given molar mass has to be calculated.

Concept Introduction:

density=PMRT

P-PressureM-MolarmassR-UniversalgasconstantT-Temperature

### Explanation of Solution

Given that:

massofthecompound=12.5mg=0.0125gvolume=125ml=0.125LPressure=24.8mmHg=0.0326atmTemperature=25°C=298K

The molar mass and molecular formula of the given boron hydride     can be calculated as

density=massvolume=0.0125g0.125L=0.1g/L

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

density=PMRT

M=dRTP=0.1g/L×0

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