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
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Secondary School Chemistry 8+4 pts
One mole of N2O4 at 300k it kept in closed container under 1 atm it is heated upto 600k when 20% mass of N2O4 decompose to NO2 .Find the resultant pressure.........
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Report by Sukant1 10.03.2018
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N2O4 → 2NO2
moles of unreacted N2O4 = 1 (1 - 0.2) = 0.8
moles of NO2 = 2 * 0.2 = 0.4
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total moles n2 = 0.8 + 0.4 = 1.2
P1/(T1 n1) = P2/(T2 * n2)
1/(300 * 1) = P2/(600 * 1.2)
P2 = 2.4 atm
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