# chemistry, first year university

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Solid NH4N3 decomposes explosively according to the following equation:

NH4N3(s) ⇌ 2N2(g) + 2H2(g)

A small amount of ammonium azide was placed in a sealed container and the air was removed. The sample was then detonated. At equilibrium the total pressure in the container was found to be 421,959.129 Pa. Calculate Kp.

• chemistry, first year university -

Assuming the temperature was at STP (0°C).

Consider a 1-L volume.
Total pressure
= 421959.129Pa
= 421.96 kPa
= 4.1654 atm at 0°C
Partial pressure of each product
= 2.08272 atm

This implies
PN2=PH2
=2.08272 atm

Kp=PN2²PH2²
= 2.0827^4
= 18.8158475075608
= 1.882*101 approx.

Note:
solids do not enter into the definition of equilibrium constants.
In any case, in an explosion, we assume all (solid) reactants have been consumed.

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