EQUILIBRIUM - A sample of 0.0020 moles of F2 was sealed into a 2.0 L reaction vessel and heated to 1000 K to study the dissociation into F atoms: F22 F At this temp., Kc=1.2x10^-4. What are [F2] and [F] at equilibrium? What is the percent dissociation of F2?

Question

EQUILIBRIUM - A sample of 0.0020 moles of F2 was sealed into a 2.0 L reaction vessel and heated to 1000 K to study the dissociation into F atoms: F2<->2 F At this temp., Kc=1.2x10^-4. What are [F2] and [F] at equilibrium? What is the percent dissociation of F2?

jfraser · Answer

do you know the general formula for an equilibrium equation?

anonymous · Answer

Kc=1.2x10^-4 and Kc=[F]^2 over [F2] so that means 1.2x10^-4=[F]^2 over [F2], right? 

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I drew an ICE table-not sure if the link above works-and plugged in .002 moles for F2 because it was given, but I'm not sure what to plug in the initial row for 2F... or if that how you even solve it