Le Châtelier’s Principle
What effect occurs when adding an inert gas to a gas-equilibrium reaction at constant volume?
What is no effect?
What is the equilibrium constant used for reactions in which solids dissolve, forming aqueous solutions?
What is Ksp?
What is the set of rules that detail the changes that occur in equilibrium (ex. when temperature is increased/decreased)?
2SO3(g) <--> O2(g) + 2SO2(g)
What is the expression for the equilibrium constant?
What is...
[O2][SO2]^2 / [SO3]^3
What is the name of the table used for finding equilibrium concentrations?
What is ICE/RICE table?
A + 2B <--> C + D
What happens if concentration of A is increased?
What is the equation shifts towards products?
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?
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?
Ka = 1.0 x 10^-4
What is the value of Kb?
What is...
Kb = 1.0 x 10^-10 ?
What is the symbol for the ratio of initial concentrations of reactants and products?
What is Q?
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?
Write the equilibrium constant for this reaction.
C2H2(g) + Cl2(g) <--> C2H2Cl(s) + HCl(g)
What is...
K = [HCl] / [C2H2][Cl2] ...?
What is the term for an ion that is common to two or more ionic compounds?
What is a common ion?
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?
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?
What is the unit of the equilibrium constant?
What is moles/L ?
What is heterogenous equilibria?
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?
Which K value has no units in its final answer?
What is Keq?
What is the only component of a reaction that, if changed, alters the value of an equilibrium concentration?
What is temperature?
What is a lower production formation?
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?
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?
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?