what volume of hydrogen at n.t.p. would be liberated by the action of 50 ml of dilute h2so4 of 40% purity and having a specific gravity of 1.3 g per ml of 65 g of zn
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Our reaction is:
Zn + H₂SO₄ ==>> H₂ + ZnSO₄
Mass of 20 ml sulfuric acid = 20 x 1.3 = 26g
1 mole (65.3g) Zn reacts with 1 mole (98g) of sulfuric acid.
So, 26g of sulfuric acid will react with =
= (65.5/98) * 26 = 17.245g of Zn only
Thus sulfuric acid is limiting reagent, so the product will depend on sulfuric acid.
So, 1 mole (98g) sulfuric acid = 1 mole hydrogen (2g)
26g of sulfuric acid = (2/98) * 26
= 0.53g
Zn + H₂SO₄ ==>> H₂ + ZnSO₄
Mass of 20 ml sulfuric acid = 20 x 1.3 = 26g
1 mole (65.3g) Zn reacts with 1 mole (98g) of sulfuric acid.
So, 26g of sulfuric acid will react with =
= (65.5/98) * 26 = 17.245g of Zn only
Thus sulfuric acid is limiting reagent, so the product will depend on sulfuric acid.
So, 1 mole (98g) sulfuric acid = 1 mole hydrogen (2g)
26g of sulfuric acid = (2/98) * 26
= 0.53g
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