A flask of volume 5 00 L is evacuated and 43 78 g of solid dinitrogen tetroxide, N 2 O 4 , is introduced at 196C The sample is then warmed to 25 C, during which time the N 2 O 4 vaporizes and some of it dissociates to form brown NO 2 gas The pressure slowly increases until it stabilizes at 2 96 atm...

A flask of volume 5.00 L is evacuated and 43.78 g of solid dinitrogen tetroxide, N 2

Question:

A flask of volume 5.00 L is evacuated and 43.78 g of solid dinitrogen tetroxide, N₂O₄, is introduced at –196°C. The sample is then warmed to 25 °C, during which time the N₂O₄ vaporizes and some of it dissociates to form brown NO₂ gas. The pressure slowly increases until it stabilizes at 2.96 atm.

(a) Write a balanced equation for the reaction.

(b) If the gas in the flask at 25°C were all N₂O₄, what would the pressure be?

(c) If all the gas in the flask converted into NO₂, what would the pressure be?

(d) What are the mole fractions of N₂O₄ and NO₂ once the pressure stabilizes at 2.96 atm?

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