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How many moles of H₂ are required to give off -9551 kJ of heat in the following reaction?
N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol

Sagot :

drpelezo

Answer:

312.1 moles H₂ (4 sig.figs. based on -9551Kj value given).

Explanation:

Given N₂(g) + 3H₂(g) => 2NH₃(g);  ΔH° = -91.8Kj*

One mole of H₂ consumed will give -91.8Kj/3 = -30.6Kj/mole (exothermic)

moles H₂ consumed that gives -9551Kj (exothermic) = -9551Kj/-30.6Kj/mole H₂

= 312.124183moles H₂ (calculator answer) ≅ 312.1 moles H₂ (4 sig.figs. based on -9551Kj value given).

*Note: The ∆H° = -91.8 kJ/mol units should be only 'Kj' as the heat flow value applies to substances with three different coefficient values in the standard equation. FYI :-)  

For the production of -9551 kJ energy, 313.55 mol of hydrogen has been consumed.

According to the balanced chemical equation,

3 moles of hydrogen have been consumed to give -91.8 kJ/mol energy.

The energy produced by 1 mole of hydrogen = [tex]\rm \dfrac{-91.38}{3}[/tex]kJ/mol

The energy produced by 1 mole of hydrogen = -30.46 kJ/mol.

For the production of -30.46 kJ/mol energy, the moles of hydrogen used are 1.

So, for the production of -9551 kJ energy, the moles of hydrogen consumed are:

- 30.46 kJ/mol = 1 mole Hydrogen

-9551 kJ = [tex]\rm \dfrac{1}{-30.46}\;\times\;-9551[/tex]

= 313.55 moles of hydrogen.

For the production of -9551 kJ energy, 313.55 mol of hydrogen has been consumed.

For more information about heat energy, refer to the link:

https://brainly.com/question/19606835

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