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 2.40 l of 0.900 m nh4no2 decomposes at 25.0°c?

Answer : The pressure of the gas will be, 5.285 atm

Solution : Given,

Volume of gas = 10 L

Temperature of gas =  

Volume of = 2.40 L

Molarity of the ammonium nitrate solution = 0.9 M

First we have to calculate the moles of ammonium nitrate.

The balanced chemical reaction is,

From the balanced reaction, we conclude that

1 mole of decomposes to give 1 mole of gas

2.16 moles of decomposes to give 2.16 moles of gas

Now we have to calculate the pressure of the gas.

using ideal gas equation,

where,

P = pressure of the gas

V = volume of the gas

T= temperature of the gas

n = number of moles of gas

R = gas constant = 0.0821 Latm/moleK

Now put all the given values in ideal gas equation, we get pressure of the gas.

Therefore, the pressure of the gas will be, 5.285 atm

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