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Alkali Metals

24.5g KClO3 i...

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24.5g KClO3 is heated to give O2 which is allowed to react completely with H2 obtained from zinc and H2SO4 reaction.the weight of Zn required for the purpose would be (Zn=65)

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Q. What mass of 60% HCl (by mass) is required to completely react with 0.2 mol of zinc and what volume of

H_{2}

will be produced at S.T.P.? The reaction is

Z n + 2 H C l \to Z n {C l}_{2} + H_{2}

Q. Equal weights of zinc and iodine react together and the iodine is completely converted to

Z n I_{2}

. What fraction by weight of the original zinc remains unreacted? (

Z n = 65, I = 127

Q. How many grams of hydrogen gas can be produced from the following reaction when

65

grams of zinc and

65

grams of HCl are allowed to react.

Z n (s) + 2 H C l (a q) \to Z n C l_{2} (a q) + H_{2} (g)

The chief ore of

Z n

is the sulphide,

Z n S

. The ore is concentrated by froth floatation process and then heated in air to convert

Z n S

Z n O

2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}

75 %

Z n O + H_{2} S O_{4} \to Z n S O_{4} + H_{2} O

100 %

2 Z n S O_{4} + 2 H_{2} O \to 2 Z n + 2 H_{2} S O_{4} + O_{2}

80 %

Z n

obtained from a sample of ore containing

292.2

Z n S

Q. The amount of zinc required to produce

1.12 mL

H_{2}

at STP on treatment with

d i l . H C l

will be: (Given: Molar mass of

Z n

65 g / m o l

)

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