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In the reaction, $4 \mathrm{NH}_3(\mathrm{~g})+5 \mathrm{O}_2(\mathrm{~g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$, When 1 mole of ammonia and 1 mole of $\mathrm{O}_2$ are made to react to completion
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All the oxygen will be consumed
\(\begin{array}{lcccc} & 4 \mathrm{NH}_{3(\mathrm{g})} & + & 5 \mathrm{O}_{2(\mathrm{g})} & \rightarrow & 4 \mathrm{NO}_{(\mathrm{g})} & + & 6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \\ t=0 & 1 & & 1 & & 0 & & 0 \\ t=1 & 1-4x & & 1-5x & & 4x & & 6x \\ \end{array}\)
Oxygen is limiting reagent
So, $\quad X=\frac{1}{5}=0.2$ all oxygen consumed
Left $N H_3=1-4 \times 0.2=0.2$.
Oxygen is limiting reagent
So, $\quad X=\frac{1}{5}=0.2$ all oxygen consumed
Left $N H_3=1-4 \times 0.2=0.2$.
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