Respuesta :
Answer:
d
Explanation:
Firstly, we need to see the theoretical mole ratio between nitrogen and ammonia from the balanced chemical equation. This is 1 to 2. One mole of nitrogen yielded two moles of ammonia.
At STP, one mole of a gas occupies a volume of 22.4, hence we need to know the volume occupied by a volume of 44.8L of ammonia. This is equal to 44.8/2 = 2 moles
Now we have seen the actual number of moles of ammonia yielded. Since this is the same as the theoretical, it means that only one mole of nitrogen was also used up.
Since it is one mole, the volume at STP is thus 22.4L
The volume of nitrogen consumed at STP has been 22.4 L. Thus, option D is correct.
The volume of an ideal gas has been given as 1 mole of gas is equivalent to 22.4 L.
The given balanced equation for Haber process has been:
[tex]\rm N_2\;+\;3\;H_2\;\rightarrow\;2\;NH_3[/tex]
Computation for volume of Nitrogen consumed
The volume of ammonia produced has been 44.8 L.
The moles of ammonia produced has been:
[tex]\rm 22.4\;L=1\;mol\\\\44.8\;L=\dfrac{1}{22.4}\;\times\;44.8\;mol\\\\ 44.8\;L=2\;mol[/tex]
The moles of ammonia produced in the reaction has been 2 mol. From the balanced chemical equation, the moles of nitrogen required to produce 2 moles of ammonia has been 1 mole.
Thus, the moles of nitrogen required has been 1 mole.
The volume of 1 mole of gas at STP has been 22.4 L. Thus, the volume of nitrogen consumed in the reaction is 22.4 L. Hence, option D is correct.
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