Question

0.26 g of a metal hydride contains 0.02g of hydrogen. What is the equivalent weight of the metal?

Answer 1

Answer:

12

Explanation:

Composition of metal hydride = 0.26g

Composition of hydrogen = 0.02

Let the atomic mass of metal be = M

Let the valency of metal be = x, then, the metal hydride will be EHx.

Thus, the molar mass of EHx = (M + x) g/mol

In metal hydride, one mole of the metal hydride contains x moles of hydrogen. Thus,

(M + x)g of metal hydride contains x g of hydrogen.

or, 0.26g of metal hydride contains x/(M + x) × 0.26 g of hydrogen.

Since, mass of hydrogen = 0.02g

or, x/(M + x) × 0.26 = 0.02

or, x/(M + x) = 1/13

or, 13x = M + x

or, 13x - x = M

or, 12x = M

or, M/x = 12

Therefore, the equivalent weight = atomic mass/valency

= M/x = 12.

Answer 2

Answer:

Explanation:

Explanation:

Composition of metal hydride = 0.26g

Composition of hydrogen = 0.02

Let the atomic mass of metal be = M

Let the valency of metal be = x, then, the metal hydride will be EHx.

Thus, the molar mass of EHx = (M + x) g/mol

In metal hydride, one mole of the metal hydride contains x moles of hydrogen. Thus,

(M + x)g of metal hydride contains x g of hydrogen.

or, 0.26g of metal hydride contains x/(M + x) × 0.26 g of hydrogen.

Since, mass of hydrogen = 0.02g

or, x/(M + x) × 0.26 = 0.02

or, x/(M + x) = 1/13

or, 13x = M + x

or, 13x - x = M

or, 12x = M

or, M/x = 12

Therefore, the equivalent weight = atomic mass/valency

= M/x = 12.