1. Tardigrade
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  3. Chemistry
  4. One mole of N2O4 gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of N2O4 decomposes to NO2(g). The resultant pressure in the container would be

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Q. One mole of $N_2O_4$ gas at 300 K is kept in a closed container at 1 atm. It is heated to 600 K when 20 percent by mass of $N_2O_4$ decomposes to $NO_2(g)$. The resultant pressure in the container would be

Chemical Kinetics

Solution:

$N_2O_4----->2 NO_2$
$Initial \, 1 \,mol$
Ateqm.$\,(1-0.2)mol \,\,0.4\,mol$
$=0.8\,mol$
Total moles after dissociation, $n_2=0-8+0-4= 1.2$
Initial temperature = 300 K $P_1 V = n_1 RT_1 or 1 \times V = 1 \times R \times 300$ ...(i) Temperature after dissociation = 600 K. No. of moles after dissociation, $n_2 = 12$ $P_2 \times V = 1.2 \times R \times 600 ...$(ii) Dividing eqn. (ii) by eqn. (i)
$p_2=\frac{1.2\times 600}{300}=2.4 atm$