Le Châtelier’s Principle
Equilibrium Constants
Unit 7 Vocab
Solving Equil. Equations
Miscellaneous
100

What effect occurs when adding an inert gas to a gas-equilibrium reaction at constant volume?

What is no effect?

100

What is the equilibrium constant used for reactions in which solids dissolve, forming aqueous solutions?

What is Ksp?

100

What is the set of rules that detail the changes that occur in equilibrium (ex. when temperature is increased/decreased)?

What is Le Chatelier's Principle?
100

2SO3(g) <--> O2(g) + 2SO2(g) 

What is the expression for the equilibrium constant?

What is...

[O2][SO2]^2 / [SO3]^3

100

What is the name of the table used for finding equilibrium concentrations?

What is ICE/RICE table?

200

A + 2B <--> C + D

What happens if concentration of A is increased?

What is the equation shifts towards products?

200

What states of matter can be used when writing the formula for an equilibrium expression? (Just Kc, no other form of K)

What are gases and aqueous solutions?

200

What do you call a reaction that takes place in both forward and reverse directions? (hint: not an equilibrium reaction)

What is a reversible reaction?

200

Ka = 1.0 x 10^-4

What is the value of Kb?

What is...

 Kb = 1.0 x 10^-10 ?

200

What is the symbol for the ratio of initial concentrations of reactants and products?

What is Q?

300

A(g) + 2B(g) <--> C(g) + D(g)

What happens if you decrease the pressure of the reaction?

What is the reaction will shift to the left/towards reactants?

300

Write the equilibrium constant for this reaction.

C2H2(g) + Cl2(g) <--> C2H2Cl(s) + HCl(g)

What is...

K = [HCl] / [C2H2][Cl2] ...?

300

What is the term for an ion that is common to two or more ionic compounds?

What is a common ion?

300

At a given temperature K = 1.3 x 10^-2 for the reaction...

N2(g) + 3H2(g) <--> 2NH3(g)

If the reaction were to be flipped, what would the value of K be?

What is 77?

300
If you increase the volume of a system at equilibrium, the reaction will shift to the side with the ____ moles of gas. 
What is most?
400

N2(g) + O2(g) <--> 2NO(g)  ΔH=-180.5 kJ

What happens to the equilibrium reaction if temperature is increased?

What is the reaction will shift towards the reactants/to the left?

400

What is the unit of the equilibrium constant?

What is moles/L ? 

400
What is the term for when equilibria involves more than one phase?

What is heterogenous equilibria?

400

The equilibrium constant Kp is 2.4x10^3 at a certain temperature for the reaction:

2NO(g) <--> N2(g) + O2(g)

The pressure of each component of the equation is: PNO=0.012 atm, PN2=0.11 atm, PO2=2.0 atm

Is the system at equilibrium? If not, which way will it shift?

What is not at equilibrium (Q>K), shifts left?

400

Which K value has no units in its final answer?

What is Keq?

500

What is the only component of a reaction that, if changed, alters the value of an equilibrium concentration?

What is temperature?

500
What does a lower value of Kc/Kp mean in terms of how much product forms?

What is a lower production formation?

500

What is the law that states that the relative concentration of reactants and products can be expressed in terms of an equilibrium constant?

What is Law of Mass Action?

500

At 35C, K=1.6 x 10^-5 for the reaction...

2NOCl(g) <--> 2NO(g) + Cl2(g)

In this reaction, there are 2 moles of NOCl in a 2L flask. Calculate the concentrations of all species at equilibrium.

What is [NO] = 0.032 M, [Cl2] = 0.016 M, and [NOCl] = 2.0 M?

500

What is the dynamic state of an equation?

What is when the reactants and products are created and used equally/when the forward rate equals the reverse rate?