A 0.2417g sample of a compound composed of C,H,O,CI only, is burned in oxygen yielding 0.4964g of CO2 and 0.0846g of H₂O. A separate 0.1696g sample of the compound is fused with sodium metal, the products dissolved in water and the chloride quantitatively precipitated with AgNO3 to yield 0.1891g of AgCl. What is the simplest empirical formula for the compound. C12H8O2Cl2 C6H5OCI C3H1002CI C6H5O2CI
A 0.2417g sample of a compound composed of C,H,O,CI only, is burned in oxygen yielding 0.4964g of CO2 and 0.0846g of H₂O. A separate 0.1696g sample of the compound is fused with sodium metal, the products dissolved in water and the chloride quantitatively precipitated with AgNO3 to yield 0.1891g of AgCl. What is the simplest empirical formula for the compound. C12H8O2Cl2 C6H5OCI C3H1002CI C6H5O2CI
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: Given data
VIEWStep 2: Calculating the mass of carbon present in carbon dioxide
VIEWStep 3: Calculating the mass of hydrogen present in water
VIEWStep 4: Calculating the mass of chlorine present silver chloride
VIEWStep 5: Calculating the mass of chlorine in the 0.2417 g of sample 1
VIEWStep 6: Calculating the mass of oxygen present in the sample
VIEWStep 7: Calculate the moles of each atom
VIEWStep 8: Calculating the mole ratio and determining the empirical formula for the compound
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