Equilibrium Constants & Concepts
With the equation: N2(g)+3H2(g) <--> 2NH3(g), can it reach equilibrium if it has 0.25 mol N2 to start with?
No. There is no H2 to form the product.
What is the difference between homogeneous and heterogeneous equilibrium?
Homogeneous has everything in the same phase. Heterogeneous has different phases.
What does it mean if Kc=Qc?
It is at equilibrium.
Find the E in the chart for Substance C.
2A+3B<--->1F+3C
2.0 M A, 0.10 B, 5.5 M F
0.0+3x
What are the four factors that affect equilibrium?
Concentration, pressure/volume, temperature, introduction of catalysts
Rates of forward and reverse reaction are equal at equilibrium. True or False?
True.
In heterogeneous equilibrium, what phase(s) of reactants and products are included in the equilibrium expression.
Gas and aqueous phase.
What is the equation relating standard Free Energy and Kc?
delta G = -RTlnK
What factor affects the direction in which the reaction proceeds AND K?
Temperature
If the reaction is product favored, is the value of Kc large or small?
Large.
What is the relationship between Kp and Kc?
Kp= Kc(RT)delta n
Q < K. Which direction does the reaction proceed?
Right (towards products)
Show us an ICE chart. CO(g)+3H2(g) <---> CH4(g)+H2O(g)
4.0 M CO, 0.10 M H2, 6.7 M H2O
See notes.
Given H2(g)+CO2(g) <---->H2O(g)+CO(g), if H2(g) is added, which direction does the reaction shift?
Right (towards products)
Write an expression for Kc. 2Hg(l)+O2(g) <---> 2HgO(s)
1 / [O2]
Find Kp. NH3(g)+H+(g)<-->NH4(g). T= 32 degrees Celsius, Kc= 4.6
0.19
What is the value of the standard Free Energy when T=40. degrees Celsius and K=0.00030?
2.1 x10 ^4
Given H2(g)+CO2(g) <---->H2O(g)+CO(g), if Ne(g) is added, how would it shift?
Solve for Kc. 2Hg(l)+O2(g) <---> 2HgO(s)
2.0 M Hg, 1.7 M O2, 0.05 M HgO
0.59
Find an expression for K3.
4NO(g)+6H2O(g) <---> 4NH3(g)+5O2(g)
2NO(g)+O2(g) <---->2NO2(g)
Overall: 4NH3(g)+7O2(g) <-----> 4NO2(g)+6H2O(g)
K3=(1/K1)(K2)2
What is the non-standard Free energy, when T=74 degrees Celsius, delta standard Free Energy=8.6 kJ and Q=3600?
32.
C2H4(g)+H2(g) <----> C2H6(g)
Show us an ICE chart and the equilibrium concentrations.
0.33 M C2H4 , 0.15 M C2H6 , Kc= 4.5.
[C2H4]=0.385
[H2]=0.0549
[C2H6]=0.205
Given H2(g)+CO2(g) <---->H2O(g)+CO(g), if the reaction is endothermic and the temperature decreases, what direction will the reaction shift?
Shifts right (towards products).