1of 2 ons14 using the following diagram and balanced equation with molecules sho

Question

1of 2 ons14 using the following diagram and balanced equation with molecules shown Before reaction After reaction 8 I. What is the limiting reactant? What is the excess reactant? What is the number of product molecules formed? 2. 4. How many molecules of the excess reactant are remaining Consider this reaction that goes rapidly to completion when ignited for questions 5-6. 2H2 +O22140 5. If our molecules of H: react, how many molecules of O: must react? 6. If 8.00 moles H: are to be reacted, how many moles of O are needed for stoichiometric equivalence? Consider the following reaction for questions 7-8

Explanation / Answer

In the given reaction it is seen that 3 moles of H2 reacts with 1 mole of N2 to produce 2 moles of NH3. Here the amount of N2 determines the amount of NH3 formed. As there are 2 N atoms in N2 and each N atoms combine with 3 H atoms from 2 H2 to form two NH3 respectively. The left over unreacted reagent is 2 atoms of H or one H2 molecule.

1) The limiting agent here is N2.

2) The excess reactant is H2.

3) 2 moles of product molecules are formed.

4) 1 molecule of H2, excess reagent, is remaining.

5) Two molecules of H2 reacts with one molecule of O2 to give 2 molecules of H2O.

Thus 4 molecules of H2 reacts with 2 molecules of O2 to give 4 molecules of H2O.

6) For 8 moles of H2, 4 moles of O2 are needed.

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