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The reaction of dimerisation of `NO_(2)` in `N_(2)O_(4)` is `2NO_(2)hArrN_(2)O_(4)`. The reaction is carried out by taking `1` mole each of `NO_(2)` and `N_(2)O_(4)` in a closed vessel of `1` litre at `400 K`. The equilibrium pressure was found to be `77 atm`. Which statements is correct for given values of teh reactions.?A. Dissociation of `N_(2)O_(4)` occurs with degree of dissociation of `N_(2)O_(4) 0.35`B. Formation of `NO_(2)` occurs and total moles of `NO_(2)` at equilibrium `1.35`C. Dissociation of `N_(2)O_(4)` occurs leaving `0.35` moles at equilibriumD. Formation of `NO_(2)` occurs with total moles at equilibrium `2.70` |
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Answer» `underset(1)(2NO_(2)) hArr underset(N_(2)O_(4))` Total moles taken `=2`, `:. P=2xx0.0821xx400=65.7 atm` Given equilibrium pressure is `77` atm, thus reaction should show the change where total number of moles increases i.e., dissociation of `N_(2)O_(4)`. `{:(N_(2)O_(4),hArr,2NO_(2)),(1,,1),(1-x,,1+2x):}` Total moles at eq.=`2+x` `=(PV)/(RT)=(77xx1)/(0.0821xx400)=2.35` `:. x=0.35` |
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