setup 1 : to the right
setup 2 : equilibrium
setup 3 : to the left
Further explanation
The reaction quotient (Q) : determine a reaction has reached equilibrium
For reaction :
aA+bB⇔cC+dD
[tex]\tt Q=\dfrac{C]^c[D]^d}{[A]^a[B]^b}[/tex]
Comparing Q with K( the equilibrium constant) :
K is the product of ions in an equilibrium saturated state
Q is the product of the ion ions from the reacting substance
Q <K = solution has not occurred precipitation, the ratio of the products to reactants is less than the ratio at equilibrium. The reaction moved to the right (products)
Q = Ksp = saturated solution, exactly the precipitate will occur, the system at equilibrium
Q> K = sediment solution, the ratio of the products to reactants is greater than the ratio at equilibrium. The reaction moved to the left (reactants)
Keq = 6.16 x 10⁻³
Q for reaction N₂O₄(0) ⇒ 2NO₂(g)
[tex]\tt Q=\dfrac{[NO_2]^2}{[N_2O_4]}[/tex]
Setup 1 :
[tex]\tt Q=\dfrac{0.0064^2}{0.098}=0.000418=4.18\times 10^{-4}[/tex]
Q<K⇒The reaction moved to the right (products)
Setup 2 :
[tex]\tt Q=\dfrac{0.0304^2}{0.15}=0.00616=6.16\times 10^{-3}[/tex]
Q=K⇒the system at equilibrium
Setup 3 :
[tex]\tt Q=\dfrac{0.230^2}{0.420}=0.126[/tex]
Q>K⇒The reaction moved to the left (reactants)
