Question

(With explanation)
2.4 g metal displaces 0.56 L H2 , at NTP, then what
would be the equivalent weight of metal?
(1) 96
(2) 48
(3) 24
(4) 12​

Answer 1

Answer:

The  correct option is (3) 24

Explanation:

From the above question, The equivalent weight of an element is its gram atomic weight divided by its valence (combining power). Some equivalent weights are: silver (Ag), 107.868 grams (g); magnesium (Mg), 24.312/2 g; aluminum (Al), 26.9815/3 g; and sulfur (S, in forming a sulfide), 32.064/2 g.

WM = 2.4 g

VH2 = 0.56 L

Let us consider the atomic weight of the metal to be 'X'. n = 40. Atomic weight (X) = equivalent weight (E) × valence (n) = 4.5 × n = 4.5 ×2 = 9.

Now,

Equivalent Mass = Mass of the Metal × 11200 Volume of Hydrogen Liberated (STP) . \text{Equivalent Mass}=\dfrac{\text{Mass of the Metal}\times 11200}{\text{Volume of Hydrogen Liberated (STP)}}. Equivalent Mass=Volume of Hydrogen Liberated (STP)Mass of the Metal×11200​. 3 3 3 grams of metal reacts with d i l X .

E = (wm * 5.6 ) / VH2

  = 2.4 * (5.6/.56)

   = 24 g

The  correct option is (3) 24

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