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Catalytic Properties

37. A sample ...

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37. A sample of KClO3 on decomposition yielded 448 mL of oxygen at STP,then the weight of KClO3 originally taken was

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{K C l O}_{3}

on decomposition yielded 448 mL of oxygen gas at NTP.
Calculate (i) Weight of oxygen product (ii) Weight of

{K C l O}_{3}

originally taken (iii) Weight of

K C l

{2 K C l O}_{3} Δ - \to {2 K C l + 3 O}_{2}

[K = 39, C = 25.5

O = 16]

0.05 g

of a commercial sample of

K C l O_{3}

on decomposition liberated just sufficient oxygen for complete oxidation of

20 m L

C O

27^{o} C

750 m m

pressure. Calculate

%

K C l O_{3}

0.05

g of a commercial sample of

K C l O_{3}

on decomposition liberated just sufficient oxygen for complete oxidation of

20

C O

27^{o} C

750

mm pressure. The percentage of

K C l O_{3}

in the sample is (as the nearest integer)

0.05

g of a commercial sample of

K C l O_{3}

on decomposition liberated just sufficient oxygen for complete oxidation of

20

C O

27

^{o} C

750

mm pressure. The

%

K C l O_{3}

in the sample is (as the nearest integer) :

Q. 1.225 g sample of

K C l O_{3}

was heated under such conditions that a part of it decomposed according to the equations given below. If the amount of

O_{2}

evolved was 168 mL at STP, calculate the weight of

K C l O_{4}

(Molar mass of K C l O_{3} = 122.5 g m o l^{- 1}, K C l O_{4} = 138.5 g m o l^{- 1}) K C l O_{3} \to K C l + O_{2} K C l O_{3} \to K C l O_{4} + K C l

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