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algol13
3 years ago
13

How many moles of potassium chloride and oxygen can be produced from 100.0g of potassium chlorate? The balanced equation is: 2 K

ClO3=2KCL+3O2
Chemistry
2 answers:
Mice21 [21]3 years ago
7 0

Answer : The moles of potassium chloride and oxygen produced can be 0.813 and 2.44 respectively.

Explanation : Given,

Mass of KClO_3 = 100.0 g

Molar mass of KClO_3 = 123 g/mole

The balanced chemical reaction will be,

2KClO_3\rightarrow 2KCl+3O_2

First we have to calculate the moles of KClO_3.

\text{ Moles of }KClO_3=\frac{\text{ Mass of }KClO_3}{\text{ Molar mass of }KClO_3}=\frac{100.0g}{123g/mole}=0.813moles

Now we have to calculate the moles of KCl and O_2.

From the balanced chemical reaction we conclude that,

As, 2 mole of KClO_3 react to give 2 mole of KCl

So, 0.813 mole of KClO_3 react to give 0.813 mole of KCl

and,

As, 2 mole of KClO_3 react to give 3 mole of O_2

So, 0.813 mole of KClO_3 react to give 3 × 0.813 = 2.44 mole of O_2

Therefore, the moles of potassium chloride and oxygen produced can be 0.813 and 2.44 respectively.

natka813 [3]3 years ago
4 0

100.0 g KClO₃ × 1 mol KClO₃/122.55 g KClO₃ × 2 mols KCl/2 mols KClO₃= 0.8160 mols of KCl

100.0 g KClO₃ × 1 mol KClO₃/122.55 g KClO₃ × 3 mols O₂/ 2 mols KClO₃= 1.224 mols of O₂

try this

122.55 g is molar mass of potassium chlorate


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What volume of oxygen gas is released at STP if 10.0 g of potassium chlorate is decomposed? (The molar mass of KClO3 is 122.55 g
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<span>KCl<span>O3</span><span>(s)</span>+Δ→KCl<span>(s)</span>+<span>32</span><span>O2</span><span>(g)</span></span>

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Note that this reaction would not work well without catalysis, typically <span>Mn<span>O2</span></span>.


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