5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the...

5.00 moles of N₂ and 8.00 moles of H₂ are placed in an empty container, the container is heated to 887 degrees Celsius, and a catalyst is added that catalyzes the rxn. of these gases to form NH₃ as the only product. At equilibrium 1.00 mole of NH₃ is found to be present. Find number of moles N₂ and moles H₂ present at equilibrium.

* I think that the concentrations of the reactants changes by 1 mole but I'm not enitrely sure if that is correct.

Expert Solution

N2 + 3 H2 <-----------------------> 2 NH3

5 8 0 ----------------------> initial

-x -3x +2x ---------------------> decomposition

5-x 8-3x 2x ---------------------------> equilibrium

equilibrium NH3 moles = 1.0

2x = 1.0

x = 0.5

equilibrium moles of N2 : 5 -x = 5 -0.5 = 4.5 mol

equilibrium moles of H2 : 8 -3x = 8 - 3 x 0.5 = 6.5 mol

queen_honey_blossom answered 7 months ago

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