What would be the change in pressure in a sealed 10.0 L vessel due to the format

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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 1.60 L of 1.50 M NH4NO2 decomposes at 25.0°C?

07 Question ( point) a See page 293 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: NH4NO2(aq ) N2(g) + 2H20 (1) 1st attempt Feedback See Periodic Table See Hint 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 1.60 L of 1.50 M NH4NO2 decomposes at 25.0°C? 3 5.88 atm

Explanation / Answer

moles of NH4NO2 reacting = M*V

= 1.50 M * 1.60 L

= 2.40 mol

According to reaction,

moles of N2 formed = moles of NH4NO2 reacted

= 2.40 mol

now use ideal gas law

Given:

Given:

V = 10.00 - 1.6 = 8.4 L

n = 2.4 mol

T = 25.0 oC

= (25.0+273) K

= 298 K

use:

P * V = n*R*T

P * 8.4 L = 2.4 mol* 0.0821 atm.L/mol.K * 298 K

P = 6.99 atm

Answer: 6.99 atm

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