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Depression in Freezing Point

52.Calculate ...

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52.Calculate the moles of pure kclo3 present in x gram of a sample of impure KCLO3 which on strong heating gives y ml of o2 at STP?

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Q. The percent loss in weight after heating a pure sample of potassium chlorate (mol.wt.=122.5) will be?
(

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

)

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

Q. Weight of 50% pure KClO3 required to produce 33.6 litres of O2 at STP is ?

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}

Q. Calculate the percent loss in weight after complete decomposition of a pure sample of potassium chlorate,

K C l O_{3} (s) \to K C l (s) + O_{2} (g)

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