The following reaction occurs readily at 425 °C: 2 NO(g) + Cl2(g) 2NOCI(g) The equilibrium constant, Kc, is 14.9 at this temperature. Suppose a reaction vessel at this temperature contained these three gases at the following 0.0500 mol/L, [C1₂] = 0.100 mol/L, [NOCI] = 0.100 mol/L concentrations: [NO] = Kc = 14.9 Show that the system is not at equilibrium. Predict the shift that the reaction would take to establish equilibrium. Briefly justify your answer.

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The following reaction occurs readily at 425 °C:
+ Cl₂(8)
2 NO
2NOCI(g)
=
The equilibrium constant, Kc, is 14.9 at this temperature.
Suppose a reaction vessel at this temperature contained these three gases at the following
0.100 mol/L, [NOCI] = 0.100 mol/L
concentrations: [NO]
0.0500 mol/L, [Ck]
Kc = 14.9
=
Show that the system is not at equilibrium. Predict the shift that the reaction would take to establish
equilibrium. Briefly justify your answer.
Transcribed Image Text:The following reaction occurs readily at 425 °C: + Cl₂(8) 2 NO 2NOCI(g) = The equilibrium constant, Kc, is 14.9 at this temperature. Suppose a reaction vessel at this temperature contained these three gases at the following 0.100 mol/L, [NOCI] = 0.100 mol/L concentrations: [NO] 0.0500 mol/L, [Ck] Kc = 14.9 = Show that the system is not at equilibrium. Predict the shift that the reaction would take to establish equilibrium. Briefly justify your answer.
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