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Decomposition - College Paper

Decomposition

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 Weight After Mass of Test tube +
KClO4 41.5g 39.8g Mass of Test tube 37.5g 37.5 Mass of KClO4
4.0g 2.3g 2. Set up the apparatus shown below.

3. Gently heat the test tube containing the potassium perchlorate. Gas should
begin to collect in the collection bottle. Record all observation. 4. Once the
reaction is complete, no more gas give off, allow the test tube to cool. While
the test tube is cooling test ...

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= .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 ŕ 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 ...

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Decomposition. (2008, December 17). Retrieved March 14, 2025, from http://www.essayworld.com/essays/Decomposition/94761

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PAPER DETAILS

Added: 12/17/2008 11:40:21 AM
Category: Science & Nature
Type: Free Paper
Words: 253
Pages: 1

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