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  3. Chemistry
  4. One mole of N2O4(g) at 300K is kept in a closed container under one atmosphere. It is heated to 600K when 20 % by mass of N2O4(g) decomposes to (NO)2(g) . The resultant pressure is Patm . Calculate the value of 10P ?

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Q. One mole of $N_{2}O_{4}\left(g\right)$ at $300K$ is kept in a closed container under one atmosphere. It is heated to $600K$ when $20\%$ by mass of $N_{2}O_{4}\left(g\right)$ decomposes to $\left(NO\right)_{2}\left(g\right)$ . The resultant pressure is $Patm$ . Calculate the value of $10P$ ?

NTA AbhyasNTA Abhyas 2022

Solution:

$\underset{1 - 0 . 2}{\underset{1}{N_{2} O_{4}}}\rightleftharpoons\underset{0 . 4}{\underset{0}{2 NO_{2}}}$
Number of moles at 300 K = 1
No. of moles at 600 K = 0.8 + 0.4 = 1.2
V is constant
$\frac{P_{2}}{P_{1}}=\frac{n_{2} T_{2}}{n_{1} T_{1}}$
$\frac{P_{2}}{1}=\frac{1.2 \times 600}{1 \times 300}=2.4atm10P=24$