Consider the following reaction Zn+2HCl→ ZnCl_2+H_2 If 520 mL of Hydrogen gas is collected over water at 28 celsius and the atmospheric pressure is 1 atm If vapour pressure of water at 28 celsius is 28.33 mm Hg. Then the amount of Zn(in gram) taken at the start of the reaction(assume all Zn(s) gets converted in product,molar mass of Zn is 65 g/mol

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Z n + 2 H C l ⟶ Z n {C l}_{2} + H_{2}

H_{2}

gas produced by the reaction is collected over water. If 0.3 g of Zn are consumed at

27^{0}

in the reaction, calculate the volume of hydrogen produced. (Given: Barometric reading=750mm, Aqueous tension at

27

=25 mm, Atomic weight of Zn=65.4).

50

c m^{3}

of hydrogen is collected over water at

17^{o}

C and

750

mm Hg pressure. Calculate the volume of dry gas at S.T.P.

[The water vapour pressure at

17^{o}

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14

mm Hg.]

A sample of $O_{2}$ gas is collected over water at 23 $^{\circ}$ C at a barometric pressure of 751 mm Hg (vapour pressure of water at 23 $^{\circ}$ C is 21 mm Hg). The partial pressure of $O_{2}$ gas in the sample collected is____.

50 c m^{3}

of hydrogen is collected over water at

17^{\circ} C

and 750 Hg pressure. Calculate the volume of dry gas at S.T.P. The water vapour pressure at

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$50 c m^{3}$ of hydrogen is collected over water at $17^{\circ} C$ and 750 mm Hg pressure. Calculate the volume of dry gas at S.T.P. The water vapour pressure at $17^{\circ} C$ is 14 mm Hg.

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