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What volume of hydrogen at N.T.P would b...

What volume of hydrogen at N.T.P would be liberated by the action of 50 mL of dilute `H_(2)SO_(4)` of 40 % purity and having a specific gravity of `1.3 g mL^(-1)` on 65 g of zinc ? (Atomic mass of Zn = 65).

Text Solution

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Step I. Calculation of mass of pure `H_(2)SO_(4)`
`"Mass of 50 mL of dilute "H_(2)SO_(4)="Volume "xx"Density = (50 mL)"xx("1.3 g mL"^(-1))=65g`
`"But 100 g of "H_(2)SO_(4)" contains pure "H_(2)SO_(4)=(40)/(100)xx65g=26g`
Step II. Calculate of volume `H_(2)` evolved at STP
The reaction taking place is
`underset("= 65 g")underset("1 mol")(Zn)+underset("= 98 g")underset("1 mol")(H_(2)SO_(4))rarrZnSO_(4)+underset("= 22.4 L at STP")underset("1 mol")(H_(2))`
Obviously, `H_(2)SO_(4)` is the limiting reagent
`"(because 20 g of Zn requires "H_(2)SO_(4)=(98)/(65)xx20" = 30 g which is not present)"`
`"98 g of "H_(2)SO_(4)" evolve "H_(2)="22.4 L at STP"`
`therefore" 26 g of "H_(2)SO_(4)" will evolve "H_(2)=(22.4)/(98)xx26=5.94L`
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