Question

Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from N₂ and H₂ by the Haber process. Because the reaction reaches equilibrium before going completely to product, the stoichiometric amount of ammonia is not obtained. At a particular temperature and pressure, 10.0 g of H₂ reacts with 20.0 g of N₂ to form ammonia. When equilibrium is reached, 15.0 g of NH₃ has formed.
(b) How many moles of N₂ and H₂ are present at equilibrium?

Answer 1

At the equilibrium we have 3.418 moles of H2 and 0.869 moles of N2

To create 2 moles of NH3 from 1 mole of N2, 3 moles of H2 are required.

We have 1.738 moles of NH3 for every 0.869 moles of N2, or 2*0.869.

Mass NH3 equals moles NH3 times molar mass NH3

17.03 g/mol of mass NH3 in 1.738 moles*

NH3 mass 29.60 grammes

Theoretical yield = NH3

calculating the yield percentage

%yield is the product of the actual yield and the theoretical yield multiplied by 100* 100%

% yield = 78.51%

There is a 78.15% yield.

At the equilibrium we have 3.418 moles of H2 and 0.869 moles of N2

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