1. Tardigrade
  2. Question
  3. Chemistry
  4. Calculate the change in pressure (in atm) when 2 mole of NO and 16 gram O 2 in a 6.25 litre originally at 27° C react to produce the maximum quantity of NO 2 possible according to the equation - 2 NO ( g )+ O 2( g ) longrightarrow 2 NO 2( g ) (Take R =(1/12) L atm / mol - K )

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Q. Calculate the change in pressure (in atm) when $2$ mole of $NO$ and 16 gram $O _{2}$ in a $6.25$ litre originally at $27^{\circ} C$ react to produce the maximum quantity of $NO _{2}$ possible according to the equation -
$2 NO ( g )+ O _{2}( g ) \longrightarrow 2 NO _{2}( g )$
(Take $R =\frac{1}{12} L atm / mol - K$ )

Equilibrium

Solution:

image
$\Delta n =|2.5-2|=0.5$
Change in pressure
$\Delta P =\frac{\Delta nRT }{ V }=0.5 \times \frac{1}{12} \times \frac{300}{6.25} atm $
$=2\, atm$