Answer
See the answer below.
Work Step by Step
From the ideal gas law:
$d=PM/RT$
$M=0.082057\ L.atm/mol.K×(25+273)\ K/(195\ mmHg×1\ atm/760\ mmHg)×1.25\ g/L $
$M=119.13\ g/mol$
Chemistry and Chemical Reactivity (9th Edition)
by Kotz, John C.; Treichel, Paul M.; Townsend, John R.; Treichel, David A.
Published by
Cengage Learning
ISBN 10:
1133949649
ISBN 13:
978-1-13394-964-0
Chapter 10 Gases and Their Properties - Study Questions - Page 403b: 26
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