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Decomposition Beginning of Paper Purpose: In this lab we will observe the products of of potassium perchlorate (KClO4). We will then predict from our results the correct chemical reaction equation. Procedure: 1. Weigh out about 4.0g of KClO4 in a test tube. Record the accurate weight below. Product Weight Before .... Middle of Paper .... forcing the water out. Burning ember re-ignited when placed into the bottle of O2. Calculations: 1. The number of moles of KClO4 that we began with is .03 moles. 4.0g ¸ 138.6g/mol = .03 moles 2. The number of moles of O2 that were present in our sample of KClO4 was .06 moles. 1.9g ¸ 32g/mole = .06 moles 3. The number of moles of O2 lost is .02 moles. 1.7g ¸ 32g/mol = .05 moles 4. KClO4 à KCl + 202 4.0g ¸ 138.6g/mol = .03 moles ´ 202 ¸ KClO4 = .06 moles ´ 32g = 1.9g 5 Percent Yield: 89% O2 lost 1.7g ¸ O2 Expected 1.9g .... 253 words | 1 pages Subscription Length Price Join 30 days membership (recurring) $19.95 90 days membership (recurring) $39.95 180 days membership (non-recurring) $69.95