Predicting if a Reaction is in Equilibrium Trial Keq Lesson 9. The Keq is a constant - a number that does not change. Changing the volume , pressure , or any concentration , does not change the Keq. Only temperature changes the Keq.

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Predicting if a Reaction is in Equilibrium Trial Keq Lesson 9

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The Keqis a constant- a number that does not change

Changing the volume, pressure, or any concentration, does notchange the Keq.

Onlytemperature changes the Keq

Increasing a [Reactant] shifts right and maintains the Keq

Increasing the temperature of an endothermic equilibrium shifts right andincreases the Keq

Ktrial

How can you tell if a system is in equilibrium or not?

Calculatea trial Keq.

Use initial concentrations in the equilibrium expression- evaluate.

How can you tell if a system is in equilibrium or not?

Calculatea trial Keq. Put initial concentrations into the equilibrium expression and evaluate.

If Kt < Keq

If Kt = Keq

If Kt > Keq

Shifts right

equilibrium

Shifts left

Kt

Kt

Kt

Keq

5

20

35

1.10.0 moles of NH3, 15.0 moles of N2, and 10.0 moles of H2 are put in a 5.0 L container. Is the system in equilibrium and how will it shift if it is not?

2NH3(g)â‡„N2(g) + 3H2(g) Keq = 10

2.0 M3.0 M2.0 M

[N2][H2]3

Kt=

=(3)(2)3

= 6

(2)2

[NH3]2

Not in equilibrium

Kt < Keq

Shifts right!

2.4.56 x 10-5 moles of NH3, 5.62 x 10-4 moles of N2, and 2.66 x 10-2 moles of H2 are put in a 500.0 mL container. Is the system in equilibrium and how will it shift if it is not?

2NH3(g)â‡„N2(g) + 3H2(g) Keq = 10

9.12 x 10-5 M1.124 x 10-5 M5.32 x 10-2 M

[N2][H2]3

Kt=

=(1.124 x 10-3 )(5.32 x 10-2 )3

= 20.3

(9.12 x 10-5)2

[NH3]2

Not in equilibrium

Kt > Keq

Shifts left!

4.If 4.00 moles of CO, 4.00 moles H2O, 6.00 moles CO2, and 6.00 moles H2 are placed in a 2.00 L container at 670 oC.