Chemistry Question

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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