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Standard XII
Chemistry
Percentage Composition
Calculate the...
Question
Calculate the mass of potassium chlorate required to liberate 6.72 of oxygen at STP.
[Assume: molar mass of potassium chlorate as 122.5 g / mol].
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Solution
2
K
C
l
O
3
⟶
2
K
C
l
+
3
O
2
From the above equation,
Amount of
K
C
l
O
3
required to liberate
(
22.4
×
3
)
L
of oxygen
=
2
×
122.5
g
Therefore,
Amount of
K
C
l
O
3
required to liberate
6.72
L
of oxygen
=
2
×
122.5
22.4
×
3
×
6.72
=
24.5
g
Hence,
24.5
g
of
K
C
l
O
3
is required.
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Q.
The percentage loss in weight after heating a pure sample of potassium chlorate will be:
[Molar mass of potassium chlorate
=
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Q.
The % loss in mass after heating a pure sample of potassium chlorate (Mol. mass = 122.5) will be:
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What is the volume of oxygen liberated at STP when 12.25 g of potassium chlorate is subjected to heating?
Q.
Potassium chlorate decomposes, on heating, to form potassium chloride and oxygen. When 24.5 g of potassium chlorate is decomposed completely, then 14.9 g of potassium chloride is formed. Calculate the mass of oxygen formed. Which law of chemical combination have you used in solving this problem?
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