Question

In some aquatic ecosystems, nitrate (NO₃^–) is converted to nitrite (NO₂^–), which then decomposes to nitrogen and water. As an example of this second reaction, consider the decomposition of ammonium nitrite:
$$NH4​NO2​(aq)N2​(g)+2H2​O(l)

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What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N₂gas when the ammonium nitrite in 2.60 L of 0.800 M NH₄NO₂ decomposes at 25.0°C?
     atm  

Answer 1

Answert The equation is NHÀ NO₂ Caq) - N₂ Cg) + 2H₂O (W) I mole of ammonium nitrate produce Imole of nitrogen gas Given that Mass of NH₃ NO₂ = 0.800 M Volume = 2.60 L no d moles of NHA NO = M XV - 0.800 M x 2.GOL = 2.08 mole Similenly, no od moles of N2 = 2.08 mole Temperature z 25° c = 25+293k = 298K Volume = 10.0L We know that Ideal gas equation we calculate the pressure PV = nRT nRT 2 - :08 mal X 0.0821 Łath md R1298K P- v - 10.0% P= 50.89 atm 100 [p = 5.089 am