CHEM 1033 Chapter Notes - Chapter 1-3: Guesstimate, Unified Atomic Mass Unit

• School: Temple University
• Department: Chemistry
• Course: CHEM 1033
• Professor: danielkim

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This experimentally-determined formula is called an empirical formula, and represents the simplest formula of the compound. General guidelines to determine the empirical formula (cid:883). (cid:883)(cid:889) (cid:883) (cid:1865)(cid:1864) (cid:883)(cid:884). (cid:882)(cid:883) =(cid:882). (cid:883)(cid:886)(cid:884) (cid:1865)(cid:1864) (cid:882). (cid:884)(cid:890)(cid:889) (cid:883) (cid:1865)(cid:1864) (cid:883). (cid:882)(cid:882)(cid:890) =(cid:882). (cid:884)(cid:890)(cid:886) (cid:1865)(cid:1864) (cid:2868). (cid:2869)4(cid:2870) (cid:2868). (cid:2869)4(cid:2870) (cid:2868). (cid:2870)48 (cid:2868). (cid:2869)4(cid:2870) (cid:2870) Thus, we can accurately represent this compound with the formula c0. 142h0. 248. Of course, per accepted convention, formulas contain whole-number subscripts, which can be achieved by dividing each subscript by the smaller subscript: Consider a sample of compound determined to contain 1. 71 g c and 0. 287 g h. the corresponding numbers of atoms (in moles) are: Avogadro"s (cid:374)u(cid:373)ber, 6. (cid:1004)(cid:1006)x(cid:1005)(cid:1004)(cid:1006)(cid:1007) (cid:373)ol 1 (or more explicitly 6. 02x1023 atoms/mol or 6. 02x1023 molecules/mol or 6. 02x1023 formula units/mol). ; and molar mass of an element or compound, the mass in grams that contains 1 mole of atoms (or molecules or formula units).