Equilibrium Position
The equilibrium shifts right when one increases one of this
Reactant
The state where the concentrations of all reactants and products remain constant with time
Equilibrium
If this is the forward reaction: aA + bB yields cC + dD. With the lower cased letters being coeffeicients and the upper cased letters being elements; this is the reverse reaction.
cC + dD yields aA + bB
In this reaction, how can I speed up the reaction without affecting the amounts in the reaction, pressure, or volume?
H2O + CO <--> H2 + CO2
Add a catalyst
**who is haber you ask?
At given temperature, Kc = 1.3 x 10^-2 for the Haber Process. Calculate the new K value if the Haber Process is halved.
0.11
The removal of a product leads to this
equilibrium shift to the products or shift right
*** no good.
When the balanced equation for a reaction is multiplied by a factor n, the equilibrium constant for the new reaction is this
Kn
If Q is equal to K then the system is at this.
Equilibrium
Calculate the Kc value for the reaction N2(g) + O2(g) -> 2NO(g) if the concentration for each individual element is as follows. N2 = .041 M, O2 = 0.0078, and NO = 4.7 x 10-4.
6.9 x 10-4
If A + B yields C + D. If A is increased, this happens to the rest of the elements. List what happens to B, C, and D.
B decreases, C increases, and D increases.
If the reaction is aA + bB yields cC + dD. K= ([C]^c [D]^d)/([A]^a [B]^b ) is the
Equilibrium Expression
For the balanced equation: aA + bB yields cC + dD
Kc= (([C]c)([D]d))/(([A]a)([B]b ))
Where is positive enthalpy written in an endothermic reaction?
Reactants / left side
These do not affect Kc. 3 things
concentration, pressure, and catalyst
If the volume of a container containing this reaction, N2(g) + 3H2(g) yields 2NH3(g), is decreased causing pressure to increase, the equilibrium shifts
shifts to the right to decrease the total molecules of gas present
These that are involved in a chemical reaction don't have their concentrations included in the equilibrium expression for the reaction
solids and liquids
These matter phases are the only ones included in the equilibrium expression.
gas(es)?
If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change
Le Chatelier's Principle
At a certain temperature, Kc = 9.1 x 10-4 for the reaction. FeSCN 2+ -> Fe3+ + SCN-. What does this tell us about the position of equilibrium for this reaction and how could we change Kc?
The reaction will favor reactants more so than products. You would need to change the temperature.
If the reaction, N2 + 3H2 yields 2NH3, produced -543 kJ of heat. If the energy is increased, this happens to the equilibrium.
equilibrium shifts left. For an exothermic system, energy is a product. The system will shift to the left to use up the excess energy
This process of Ammonia from Nitrogen and Hydrogen is called
The Haber Process
Balance this equation and determine its equilibrium expression: Hydrogen + Bromine yields Hydrobromic Acid. All of these elements are gases.
([HBr]2)/([H2][Br2])
Name two ways to change the pressure of the system
add or remove a gaseous product or reactant, change the temperature or change the volume of the container
A <---> B
A starts out with 1 mole. It reacts at 60% a minute.
B starts out with 1 mole. It reacts at 20% a minute.
ROUND TO THE NEAREST TENTH. How long until equilibrium?
2 minutes