Description
particular temperature, Kp = 0.260 reaction
N2O4(g) 2NO2(g)With no change amount material in flask, the volume container question increased to 5.000 times original. Assuming constant temperature,calculate (new) total pressure, at equilibrium.
Explanation & Answer
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It
makes no difference whether you increase 5times the volume after at the
equlibrium established in (1) of you start start the reaction from
initial pure nitrogen dioxide in a 5times bigger volume flask.
increasing the volume 5 times original means halving the initial pressure to
p₀/592 inHg
so normal atmosphere pressure= 29.92 in Hg
so initial pressure becomes = 29.92/5 =5.984
The partial fulfill equilibrium condition:
Kp = (p(NO2))² / p(N2O4)
Kp = (p₀ - 5·Δp)² / Δp
now we have Kp=0.26 and p0=5.984
now find out Δp
0.26 = p0^2 +25 Δp^2 -1op0 Δp
25 Δp^2 - 10.26 p0 Δp + p0^2=0
25 Δp^2 - 61.4 Δp +35.81 =0
find the value of Δp
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