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Question

# One mole of N2O4(g) at 300 K is left in a closed container under one atm. It is heated to 600 K when 20% by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is:

A
1.2 atm
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B
2.4 atm
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C
2.0 atm
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D
1.0 atm
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Solution

## The correct option is A 2.4 atmGiven:Decomposition of N2O4 is 20% by mass. 1 mole ⇒ 28gmass decomposed =28×20100=5.6g mass left after decomposition =28−5.6=22.4No. of moles of N2O4 left=22.428=0.8 moleN2O4⇋2NO2 N2O4 NO2 Initial moles10 Change moles −0.20.4 Equilibrium pressure 0.80.4 Total number of moles =0.8+0.4=1.2Pressure at 300 K is 1 atm.Pressure at 600 K (without considering decomposition) will be P2=T2×P1T1=600×1300=2 atm.Total pressure (when decomposition is considered) =2×Final total number of molesInitial total number of moles=2×1.21=2.4 atm.

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