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Alkali Metals

24.5g KClO3 i...

Question

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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