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WorksheetsChemical Equilibrium
Total questions: 37
Worksheet time: 38mins
The forward reaction forms the substance __________.
The reverse reaction points towards the __________.
A complete reaction is in which:
All the reactants convert into products
All the reactants do not convert into products
Half reactants convert into products
only 10% reactants convert into products
Removing O2(g) will
Adding SO2(g) will
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
Decreasing volume of container will
H2(g)+Cl2(g)⇌2HCl(g)
Increasing the pressure will
shift equilibrium right
shift equilibrium left
You cannot predict the effect
have no change
H2(g)+Cl2(g)⇌2HCl(g)
The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?
equilibrium shifts right
equilibrium shifts left
You cannot predict the effect
no change
What kind of equilibrium does the reaction below show?
H2(g) +I2(g) ↔ 2HI(g)
Heterogeneous equilibrium, all the reactants and products are in the same physical state.
Homogeneous equilibrium, all the reactants and products are in the same physical state.
Heterogeneous equilibrium, the reactants and products are present in more than one physical state
Homogeneous equilibrium, the reactants and products are present in more than one physical state
heat + N2 + O2 <−> 2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium
the reactants are favored.
the products are favored.
approximately equal concentrations of reactants and products are present.
When pressure decreases, in which direction does the equilibrium shift?
The equilibrium shifts in the direction that increases the number of moles of gas.
The equilibrium shifts in the direction that decreases the number of moles of gas.
The equilibrium does not shift.
The equilibrium shifts always shifts to the right.
The equilibrium shifts always shifts to the left.
For an endothermic reaction, increasing the temperature
does not shift the equilibrium since K is a constant.
increases the rate of the reverse reaction to form more reactants.
increases the rate of the forward reaction to form more products.
increases the rate of the reverse reaction to form more products.
What is the value for Kc if [CO] = 0.025, [H2] = 0.013 and [CH3OH] = 0.0028 for the following reaction?
CH3OH(g) ⇌ CO(g) + 2 H2(g)
0.12
9.1 × 10-7
6.6 × 102
1.5 × 10-3
8.6
For the reaction PCl5 (g) → PCl3 (g) + Cl2 (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl5] = 0.25M, [PCl3] = 0.20 M, and [Cl2] = 2.25 M, in which direction will a reaction occur and why?
toward products because Q = 0.56
toward reactants because Q = 1.8
it is at equilibrium
toward reactants because Q = 0.0454
toward products because Q = 2.8
Consider the following reaction.
C(s) + H2O(g) ⇌ CO(g) + H2(g)
At equilibrium at a certain temperature, [H2O(g)] = 0.12 M, and [CO(g)] = [H2(g)] = 1.2 M. If suddenly these concentrations are increased by 0.50 M, which of the following is true?
Since Kc does not change, nothing happens.
more products are formed
more H2O(g) will be formed
Kc = 4.66
For the reaction: CH4(g) + 2 H2O(g) ⇔ CO2(g) + 4 H2(g) ΔH° = +190 kJ raise the temperature to 1200 K:
the temperature increases.
the ΔH° increases.
the reaction reacts to the right.
the reaction reacts to the left.
there is no change.
Consider the reaction: CH4(g) + 4 Cl2(g) ⇔ CCl4(l) + 4 HCl(g) ΔH° -398 kJ/mol The equilibrium is displaced to the right if:
the pressure is lowered
the temperature is raised
some hydrogen chloride is added
some hydrochloric acid is removed
Choose the correct statement about a container in which the chemical equilibrium is established:
2 SO2(g) + O2(g) → 2 SO3(g) + heat
A decrease in the volume will decrease the amount of SO2 present.
An increase in amount of O2 will increase the amount of SO2 present.
A decrease in temperature will increase the amount of SO2 present.
A decrease in the amount of SO3 present will increase the amount of SO2 present.
A decrease in amount of O2 will decrease the amount of SO2 present.
For a reaction Keq = 1.2 × 10-6 at T = 200 K. What is ΔG° for the reaction?
-22.7 kJ/mol
22.7 kJ/mol
53.6 kJ/mol
170 kJ/mol
-53.6 kJ/mol
Calculate the temperature for which Keq for a reaction is 1.04 × 103 where ΔH° = -83.2 kJ/mol and ΔS° = -246 J/mol ∙ K.
0.307 K
307 K
274 K
0.274 K
cannot be determined without ΔG°
Given N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g), which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?
Place only N2 into a sealed vessel.
Place only H2 into a sealed vessel.
Place only NH3 into a sealed vessel.
none of the above
Le Chatelier's Principle states that:
a disturbing force must be applied to a system in order for it to reach equilibrium.
when a system at equilibrium is disturbed, a new equilibrium constant is established.
when a chemical system at equilibrium is disturbed, the system shifts in order to minimize the effect.
when a chemical system is at equilibrium it is no longer possible to alter the system.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
[Fe]3 [H2O]4 / [Fe3O4] [H2]4
[Fe3O4] [H2]4 / [Fe]3 [H2O]4
[H2O]4 / [H2]4
[Fe] [H2O] / [Fe3O4] [H2]
A catalyst is added to a system at equilibrium.
The concentration of the reactants will then
decrease
increase
remain the same
approach zero
none of the above
A solution at equilibrium must be
concentrated
saturated
unsaturated
diluted
If QC > KC , in order to achieve chemical equilibrium, the reaction shift to the
Left
Right
Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?
Divide Kc by 1
Divide 1 by Kc
Square Kc
Take the square root of Kc
