Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question

Transcribed Image Text:CH4
C2H3
C3H12
C4H16
II
IV
Chemical analysis of a gaseous compound showed that it contained 75.0 percent carbon (C)
and 25.0 percent hydrogen (H) by mass.
At 200°C, 97.2 L of the compound exerted a pressure of 0.74 atm.
If the mass of 97.2 L of the compound was 59.2 g, calculate the molecular formula of the
compound. (Molar mass of C is 12 g/mole, molar mass of H is 1 g/mole)

Transcribed Image Text:The average atomic mass of hypothetical element 71X
(70.9247 amu) and 67X (66.9256 amu) is 69.72 amu.
Calculate the natural abundances of the X isotopes.
A- 71X 60.3 %
67X 39.7 %
В- 71X 39.7 %
67X 60.3 %
С-71х 29.7%
67X 70.3 %
D- 71X 69.9 %
67X 30.1 %
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