The change in pressure in a sealed 10.0L vessel is 5.28 atm
<u><em>calculation</em></u>
The pressure is calculated using the ideal gas equation
That is P=n RT
where;
P (pressure)= ?
v( volume) = 10.0 L
n( number of moles) which is calculated as below
<em>write the equation for decomposition of NH₄NO₂</em>
NH₄NO₂ → N₂ +2H₂O
<em>Find the moles of NH₄NO₂</em>
moles = molarity x volume in liters
= 2.40 l x 0.900 M =2.16 moles
<em>Use the mole ratio to determine the moles of N₂</em>
that is from equation above NH₄NO₂:N₂ is 1:1 therefore the moles of N₂ is also =2.16 moles
R(gas constant) =0.0821 l.atm/mol.K
T(temperature) = 25° c into kelvin = 25 +273 =298 K
make p the subject of the formula by diving both side by V
P = nRT/V
p ={ (2.16 moles x 0.0821 L.atm/mol.K x 298 K) /10.0 L} = 5.28 atm.
