1. Tardigrade
  2. Question
  3. Chemistry
  4. Consider the following reaction equilibrium N2(g)+3H2(.g.)leftharpoons2NH3(.g.) Initially, 1 mole of N2 and 3 moles of H2 are taken in a 2 L flask. At equilibrium state if, the number of moles of N2 is 0.6, what is the total number of moles of all gases present in the flask?

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Q. Consider the following reaction equilibrium

$N_{2}\left(g\right)+3H_{2}\left(\right.g\left.\right)\rightleftharpoons2NH_{3}\left(\right.g\left.\right)$

Initially, 1 mole of $N_{2}$ and 3 moles of $H_{2}$ are taken in a 2 L flask. At equilibrium state if, the number of moles of $N_{2 \, }$ is 0.6, what is the total number of moles of all gases present in the flask?

NTA AbhyasNTA Abhyas 2020Equilibrium

Solution:

Solution

Number of moles of $\text{N}_{2}=0.6=1-\text{x}$

$\therefore $ $\text{x}=1-0.6=0.4$

So, $3-3\text{x}=3-3\times 0.4=1.8$ ,

and $2\text{x}=2\times 0.4=0.8$

Therefore, the total number of moles at equilibrium.

$=\left(1 - \text{x}\right)+\left(3 - 3 \text{x}\right)+2\text{x}$

$=0.6+1.8+0.8$

$=3.2$ mol