Answer: 0.5 moles
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
[tex]4NH_3+3O_2\rightarrow 2N_2+6H_2O[/tex]
According to stoichiometry,
4 moles of ammonia produce = 2 moles of nitrogen
1 mole of ammonia produce =[tex]\frac{2}{4}\times 1=0.5[/tex] moles of nitrogen
Thus 0.5 moles of nitrogen are consumed when 1 mole of ammonia is consumed.
The number of moles of N₂ produced when 1.0 mole of NH₃ is consumed is 0.5 moles
From the question, the given reaction is
4NH3 + 3O2 → 2N2 + 6H2O
First, we will rewrite the equation for the reaction properly
The balanced equation for the reaction written properly is
4NH₃ + 3O₂ → 2N₂ + 6H₂O
Now, to determine the number of moles of N₂ that are produced when 1.0 mole of NH₃ is consumed,
From the balanced chemical equation given
4 moles of NH₃ reacts with 3 moles of O₂ to produce 2 moles of N₂ and 6 moles of H₂O
That means
4 moles of NH₃ will produce 2 moles of N₂
Now,
If 4 moles of NH₃ will produce 2 moles of N₂
Then, 1.0 mole of NH₃ will produce [tex]\frac{2}{4}[/tex] moles of N₂
∴ Number of moles of N₂ produced [tex]=\frac{2}{4} = \frac{1}{2}= 0.5\ moles[/tex]
Hence, the number of moles of N₂ produced when 1.0 mole of NH₃ is consumed is 0.5 moles
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