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# Solved: Calculating Amounts of Reactants and Products ISBN: 9780321809247 1

## Solution for problem 2PE Chapter 3.16SE

Chemistry: A Molecular Approach | 3rd Edition

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Problem 2PE

Calculating Amounts of Reactants and Products Determine how many grams of water are produced in the oxidation of 1.00 g of glucose, C6H12O6: Decomposition of KCLO3 is sometimes used to prepare small amounts of O2 in the laboratory: 2KCLO3(s)? 2kcl + 3O2.(g) . How many grams of O2 can be prepared from 4.50 g of KCLO3?

Step-by-Step Solution:

Answer Step 1 Given the reaction on the basis of molar mass Here the reaction is 2KClO3(S) 2KCl + 3O2(g). We have to convert 4.50 kg of KCIO3 to moles of KCLO3 by using molar mass of KCLO3 Molar mass of KCLO3=122.5g/mol Moles of KCLO3=4.50g/122.5 g/mol =0.0367 moles.

Step 2 of 2

##### ISBN: 9780321809247

Since the solution to 2PE from 3.16SE chapter was answered, more than 356 students have viewed the full step-by-step answer. The answer to “Calculating Amounts of Reactants and Products Determine how many grams of water are produced in the oxidation of 1.00 g of glucose, C6H12O6: Decomposition of KCLO3 is sometimes used to prepare small amounts of O2 in the laboratory: 2KCLO3(s)? 2kcl + 3O2.(g) . How many grams of O2 can be prepared from 4.50 g of KCLO3?” is broken down into a number of easy to follow steps, and 56 words. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. The full step-by-step solution to problem: 2PE from chapter: 3.16SE was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. This full solution covers the following key subjects: kclo, amounts, grams, oxidation, glucose. This expansive textbook survival guide covers 82 chapters, and 9454 solutions.

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Solved: Calculating Amounts of Reactants and Products