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3. What mass of O₂ can theoretically be obtained from 1.67 g of a KClO3/KCl mixture which is 75.0% by weight KClO3?

3. What mass of O₂ can theoretically be obtained from 1.67 g of a KClO3/KCl mixture which is 75.0% by weight KClO3?

Chemistry
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
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**Question 3:** What mass of \( \text{O}_2 \) can theoretically be obtained from 1.67 g of a \( \text{KClO}_3/\text{KCl} \) mixture which is 75.0% by weight \( \text{KClO}_3 \)?
Transcribed Image Text:**Question 3:** What mass of \( \text{O}_2 \) can theoretically be obtained from 1.67 g of a \( \text{KClO}_3/\text{KCl} \) mixture which is 75.0% by weight \( \text{KClO}_3 \)?
Expert Solution
Step 1

#3:

Between KCl and KClO3, only KClO3 is decomposed to form O2(g). 

The balanced equation for the decomposition reaction is:

2KClO3(s) → 2KCl(aq) + 3O2(g)

The required mole ratio is:

3 mol O22 mol KClO3

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