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WorksheetsTrial UPS Chapter 6: Chemical Equilibrium
Total questions: 20
Worksheet time: 10mins
For the reaction...
SO2 (g) + O2 (g) ⇌ SO3(g)
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
left
right
left and right
neither left nor right
For the reaction...
N2 (g) + 3 H2(g) ⇌ 2 NH3 (g)
If the pressure in the system is increased, which substance(s) will increase in concentration?
N2
H2
N2 and H2
NH3
Removing O2(g) will
Which of the following is NOT true at equilibrium?
The forward and reverse reactions proceed at the same rate.
The concentrations of reactants and products do not change.
The concentration of the reactants is equal to the concentration of the products.
The forward and reverse reactions continue to occur.
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
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]
Shift Left (towards reactants)
Shift Right (towards products)
Speed up the reaction and shift the equilibrium
Speed up the reaction and NOT affect equilibrium
Shift towards the side with LESS moles
Shift towards the side with MORE moles
Speed up the reaction and shift the equilibrium
Speed up the reaction and NOT affect equilibrium
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
2SO3(g) ↔ 2SO2(g) + O2(g)
Kc = 4.08x10-3 at 1000K
What is Kp?
Which factor will effect the change in equilibrium constant?
Pressure
Concentration
Add inert gas
Temperature
Predict the change in equilibrium position when Ne gas is added at constant volume to an equilibrium system.
Equilibrium position remain unchanged.
Equilibrium shift to the side with more number of moles.
Equilibrium position shift to the right.
Equilibrium shift to the side with less number of moles.
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.
PCl3 (g) + Cl2 (g) ↔ PCl5 (g) + HEAT
Which of the following causes an increase in equilibrium constant, K?
Increase in pressure
Increase in temperature
Decrease in temperature
Increase the concentration of PCl3
