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Studentka2010 [4]
2 years ago
5

The decomposition of potassium chlorate yields oxygen gas. If the yield is 85%, how many grams of KClO3 are needed to produce 15

.0 L of O2 ?
2KClO3(s) -- > 2KCl(s) + 3 O2(g)
Chemistry
2 answers:
Harlamova29_29 [7]2 years ago
6 0

Answer:

m_{KClO_3}=64.4gKClO_3

Explanation:

Hello,

At first, the undergoing chemical reaction is:

2KClO_3(s)-->2KCl(s)+3O_2(s)

As 15.0 L of oxygen were produced, one computes this amount in moles considering STP conditions (0°C and 1 atm) for the ideal gas equation as shown below:

n_{O_2}=\frac{PV}{RT} =\frac{1atm*15.0L}{0.082 \frac{atm*L}{mol*K} *273.15K}=0.670molO_2

Now, since those moles are the actual obtained moles, one computes the theoretical moles of oxygen which are more precisely associated with the needed grams of potassium chlorate as follows:

n_{O_2}^{Theoretical}=\frac{0.670molO_2}{0.85} =0.788molO_2

Finally, we apply the stoichiometry to determine the moles of potassium chlorate as shown below:

m_{KClO_3}=0.788molO_2*\frac{2molKClO_3}{3molO_2} *\frac{122.55gKClO_3}{1molKClO_3} \\m_{KClO_3}=64.4gKClO_3

Best regards.

Novosadov [1.4K]2 years ago
5 0
 <span>2KClO3 = 2KCl + 3O2. 

10 L are 10/22.4 moles as 1 mole of gas at STP occupies 22.4 L so 0.446 moles but you only get 95% yield so you need to make more than 0.446 moles -- you need 0.446/0.95 = 0.470 moles. 

Two moles KClO3 give 3 moles O2 so you need 0.470*(2/3) moles KClO3 = 0.313 moles KClO3 and that has molar mass = 39 + 35.5 + 3*16 = 122.5 g so in g 0.313*122.5 = 38.4 g KClO3</span><span>
</span>
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