One mole of (g) at 300 K is kept in a closed container under 1 atmospheric pressure. It is heated to 600 K when 20% by mass of (g) decomposes to (g). The resultant pressure is [5]

Question

One mole of $N_2O_4$(g) at 300 K is kept in a closed container under 1 atmospheric pressure. It is heated to 600 K when 20% by mass of $N_2O_4$(g) decomposes to $NO_2$(g). The resultant pressure is [5]

Prashant Kotian · Accepted Answer

Correct answer: B. Reaction: (g) ⇌ 2 (g). Since 20% decomposes, α = 0.2. Total moles at equilibrium = n*(1 + α) = 1 * 1.2 = 1.2 moles. From the gas law: P2 = P1 * (n2/n1) * (T2/T1) = 1 * (1.2/1.0) * (600/300) = 2.4 atm. [5]

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