WorksheetsEquilibrium and K
Total questions: 15
Worksheet time: 1hrs 15mins
Which is the correct equilibrium constant expression for the following reaction?
Fe2O3(s) + H2(g) —> Fe(s) + H2O(g)
K = [H2O]3 / [H2]3
K = [Fe2O3] [H2]3 / [Fe]2[H2O]3
K = [Fe]2[H2O]3 / [Fe2O3] [H2]3
K= [Fe] [H2O] / [Fe2O3] [H2]
K = [H2] / [H2O]
The equilibrium constant expression for the reaction BrF5(g) —> Br2(g) + F2(g) is
Kc = [Br2] [F2] / [BrF5]
Kc = [BrF5]2 / [Br2][F2]5
Kc = [Br2] [F2]5 / [BrF5]2
Kc = 2[BrF5]2 / ([Br2] × 5[F2]5)
Kc = [Br2] [F2]2 / [BrF5]5
The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2(g) + H2O(l) —> H2CO3(aq)
Which one of the following is the correct equilibrium constant expression (Kc) for this reaction?
Kc= 1/ [H2CO3]
Kc= [CO2]/ [H2CO3]
Kc= [H2CO3] / [CO2]
Kc= [CO2] [H2O] / [H2CO3]
Kc= [H2CO3] / [CO2] [H2O]
Calculate Kc for the reaction HI(g) —> H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27mol/L.
0.19
0.22
4.5
5.25
160
A chemical reaction in which products can react to re-form reactants is known as a(n)
reforming reaction
reversible reaction.
buffered reaction
stoichiometric reaction.
For any reaction at chemical equilibrium, the concentrations of products and reactants
are equal.
change
remain unchanged
decrease
A very high value for K indicates that
reactants are favored.
products are favored.
equilibrium is reached slowly.
equilibrium has been reached
This symbol indicates that a reaction is _____
reversible
irreversible
Around what time does the reaction reach equilibrium?
25 min
70 min
45 min
80 min
Which of the two graphs reaches equilibrium?
Neither
The left
Both
The right
What states of matter are omitted when writing Keq expressions?
solids and liquids
aqueous solutions and gas
solids, liquids, aqueous solutions and gases
aqueous solutions & liquids
When Keq < 1,
There are more products than reactants when the reaction reached equilibrium.
There are more reactant than products when the reaction reached equilibrium.
The amount of reactants is equal to the amount of products.
What is the Keq expression for this reaction?
2 NO(g) + O2(g) ⇌ 2 NO2(g)
Kc = [NO2]2 / [NO]2 [O2]
Kc = [NO]2 [O2] / [NO2]2
Kc = [NO]2 [O2] [NO2]2
Kc = [NO2]2 / [NO]2 + [O2]
The following reaction :
SO2 (g) + NO2 (g) ⇌ SO3 (g) + NO (g)
established equilibrium and was found to contain
0.40 M SO3 , 0.30 M NO,
0.15 M NO2 , and 0.20 M SO2.
Calculate the equilibrium constant for this reaction.
4.0
.42
.25
1.0
Calculate [H2O] if Keq = 1.2,
[CO2] = 0.846M, and [CH4]= 0.0713M
4CuO(s) +CH4(g) ⇌ CO2(g)+4Cu(s) +2H2O(g)
0.101 M
0.318 M
0.0102 M
3.77 M
