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Equilibrium constant calculation help.
I'm having trouble working out this question:
The equilibrium constant for the reaction
2NO2(g) ⇌ 2NO(g) + O2(g)
is 9 moldm-3 at 683K
equilibrium concentrations were measured as
NO(g) = 0.5 moldm-3
O2(g) = 0.25 moldm-3
What is the equilibrium concentration of NO2(g) in the above mixture.
I know the answer is 0.083 but I can't get to it.
+REP
The equilibrium constant for the reaction
2NO2(g) ⇌ 2NO(g) + O2(g)
is 9 moldm-3 at 683K
equilibrium concentrations were measured as
NO(g) = 0.5 moldm-3
O2(g) = 0.25 moldm-3
What is the equilibrium concentration of NO2(g) in the above mixture.
I know the answer is 0.083 but I can't get to it.
+REP
Okay so:
and 9 = [0.5]2[0.25]/[NO2]2
so rearrange so that [NO2]2 = [0.5]2[0.25]/9
then take the square root
and 9 = [0.5]2[0.25]/[NO2]2
so rearrange so that [NO2]2 = [0.5]2[0.25]/9
then take the square root
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