Consider the reaction: 2 NO (g) + 5 H2 (g) → 2 NH3 (g) + 2 H2O (g) A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Which set of amounts best represents the mixture after the reactants have reacted as completely as possible?

Question

Jasiah Garner

Chemistry

23 July, 03:34

Consider the reaction: 2 NO (g) + 5 H2 (g) → 2 NH3 (g) + 2 H2O (g) A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Which set of amounts best represents the mixture after the reactants have reacted as completely as possible?

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Evelin · Answer 1

2 NO (g) + 5 H2 (g) → 2 NH3 (g) + 2 H2O (g)

From the reaction above, 2 moles of NO requires 5 moles of H2 to obtain 2 moles of NH3 and 2 moles of H2O

If all the 5 moles of NO was used, it would require;

2 moles of NO = 5 moles of H2

5 moles of NO = x

x = 12.5 moles of H2

However there is only 10 moles of H2. This makes it the limiting reactant.

When the 10 moles of H2 are used;

5 moles of H2 = 2 moles of NO

10 moles of H2 = x

x = 4 moles of NO

This means 4 moles of NO and 10 moles of H2 are used.

Only 1 mole of NO would remain.