Respuesta :

Answer : The mass of [tex]H_2[/tex] is, 9.64 grams.

Explanation : Given,

Mass of [tex]NH_3[/tex] = 54.6 g

Molar mass of [tex]NH_3[/tex] = 17 g/mol

Molar mass of [tex]H_2[/tex] = 2 g/mol

First we have to calculate the moles of [tex]NH_3[/tex].

[tex]\text{Moles of }NH_3=\frac{\text{Given mass }NH_3}{\text{Molar mass }NH_3}[/tex]

[tex]\text{Moles of }NH_3=\frac{54.6g}{17g/mol}=3.21mol[/tex]

Now we have to calculate the moles of [tex]H_2[/tex]

The balanced chemical equation is:

[tex]2NH_3(g)\rightarrow 3H_2(g)+N_2(g)[/tex]

From the balanced reaction we conclude that

As, 2 mole of [tex]NH_3[/tex] react to give 3 moles of [tex]H_2[/tex]

So, 3.21 mole of [tex]NH_3[/tex] react to give [tex]\frac{3}{2}\times 3.21=4.82[/tex] mole of [tex]H_2[/tex]

Now we have to calculate the mass of [tex]H_2[/tex]

[tex]\text{ Mass of }H_2=\text{ Moles of }H_2\times \text{ Molar mass of }H_2[/tex]

[tex]\text{ Mass of }H_2=(4.82moles)\times (2g/mole)=9.64g[/tex]

Therefore, the mass of [tex]H_2[/tex] is, 9.64 grams.

samueladesida43

9.6 grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction: 2NH₃(g) → 3H₂(g) + N₂(g).

  • According to this question, the following balanced equation is given: 2NH₃(g) → 3H₂(g) + N₂(g).

  • First, we convert the mass of ammonia (NH3) to moles as follows:

  • moles of NH3 = 54.6g ÷ 17g/mol

  • moles of NH3 = 3.2mol.

  1. If 2 moles of NH3 produces 3 moles of H2.
  2. 3.2 moles of NH3 will produce 4.8 moles of H2.

  • Next, we convert 4.8moles of H2 to mass as follows:

  • mass of H2 = 4.8 × 2

  • mass of H2 = 9.6g of H2.

  • Therefore, 9.6 grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction: 2NH₃(g) → 3H₂(g) + N₂(g).

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