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) + 3SO2(g)
What is the expression for the equilibrium constant?
What is...
[O2][SO2]3 / [SO3]2
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?
The reaction 2NO2 (g) <--> N2O4 (g) is an exothermic reaction. NO2 is brown while N2O4 is colorless. If the reaction is light brown at equilibrium, predict the changes to the color when the reaction is cooled.
What is...
The color will become lighter as there will be a shift towards the products.
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 the inverse of K (1/1.3 x 10-2) ?
If you increase the volume of a system at equilibrium, the reaction will shift to the side with the ____ moles of gas.
What is more?
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 equilibrium constant does not have units.
What is heterogenous equilibria?
The equilibrium constant Kp is 2.4x103 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?
When will a precipitate form in a solubility equilibrium reaction?
What is when Q > K?
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 constant is used when a reaction is not at equilibrium?
What is reaction quotient (Q)?
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?