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: What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N2 gas when the ammonium nitrite in 2.20 L of 1.10 M NH4NO2 decomposes at 25.0°C?

Question

Meredith Massey

Chemistry

7 April, 18:37

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: What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N2 gas when the ammonium nitrite in 2.20 L of 1.10 M NH4NO2 decomposes at 25.0°C?

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Kathy Cooper · Answer 1

The equation is:

NH₄NO₂ (aq) → N₂ (g) + 2H₂O (l)

The moles of NH₄NO₂ (aq) is:

M ₓ V = 1.10 ₓ 2.20 = 2.4 moles of NH₄NO₂

1 mole of NH₄NO₂ = 1 mole of N₂

2.4 mole = 2.4 mole of N₂

No liquid volume = V total - V liquid = 10 - 2.20 = 7.8 liters.

Now, substituting the data in the equation PV = nRT we get:

PV = nRT

P = nRT/V

P = 2.4 ₓ 0.082 ₓ 298 / 7.8

P = 7.5 atm