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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Step 1
Assuming the empirical formula of the compound is CaHbOc.
Given : Mass of CO2 produced = 0.4261 g
Mass of H2O produced = 0.1744 g
Molar mass of CO2 = Atomic mass of C + Atomic mass X 2 = 12 + 16 X 2 = 44 g/mol
And molar mass of H2O = Atomic mass of H X 2 + Atomic mass of O = 1 X 2 + 16 = 18 g/mol
Since mass = moles X molar mass
=> 0.4261 = moles of CO2 X 44
=> moles of CO2 produced = 9.684 X 10-3 mol approx.
And 0.1744 = moles of H2O X 18
=> moles of H2O produced = 9.688 X 10-3 mol approx.
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