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Le Chatelier's Problem Solving
Equilibrium Graphs
Equilibrium Constant (Keq)
NO CHEMISTRY HERE
100
Is this equation an endothermic or Exothermic reaction?
NaOH + HCI → NaCI + H2O ΔH= +122kj
endothermic
100
The following reaction is allowed to reach equilibrium.
COBr2(g)⇌CO(g)+Br2(g)
What happens to the reaction when inert argon gas, Ar(g), is added?
Nothing happens/ reaction still at equilibrium.
100
What disturbance likely occurred at time (t). 
Temperature decrease
100
What is the Keq equation for
N2(g) +3H2(g) <—> 2NH3(g)
Keq = [NH3]2 /[N2][H2]3
100
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200
What is the effect of adding a catalyst to a reaction in equilibrium?
It increases the forward and reverse reactions equally, and thus doesn’t alter the position of equilibrium.
200
The following exothermic reaction is allowed to reach equilibrium.
2H2(g)+O2(g) ⇌ 2H2O(g) + HEAT
What happens to the reaction when the temperature is decreased?
Shift right - Favors forward reaction
200
What stress has likely occurred in this system?
Temperature increase
200
When Keq > 1 which side of the reaction is favoured?
Products/Right Side
200
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The Legend of Zelda: Tears of the Kingdom?
300
Consider the reaction:
A(g) + B(g) ⇋ C(g)
In an equilibrium mixture the following concentrations were found:
[A] = 0.45M, [B] = 0.63M and [C] = 0.30M.
Calculate the value of the equilibrium constant for this reaction.
Keq = 1.1
300
What is the affect of adding a catalyst to an equilibrium reaction?
Increases the forward and reverse reactions equally, meaning no change in the position of equilibrium
300
N2(g)+3H2(g)⇌2NH3(g) ΔH=−92kJmol−1
What happened at t1?
N2 gas was added
300
What is the equilibrium constant K for the chemical equation:
ClNO2(g)+NO(g)<—>NO2(g)+ClNO(g)
K=[NO2][ClNO]/[ClNO2][NO]
300
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400
Both of these graphs show a reaction at equilibrium. For each of the graphs, how would we label the y axis?
Top Graph - Rate
Bottom Graph - Concentration
400
Consider the equation:
BaCl2 (aq) + NaSO4 (aq) <--> 2NaCl (aq) + BaSO4 (s)
If barium chloride (BaCl2) is added to the system, what change occurs?
The reaction shifts to the right, which results to an increase in the yield of products.
400
N2(g)+3H2(g)⇌2NH3(g) ΔH=−92kJmol−1
What happened at t2?
Volume was decreased (increase in pressure)
400
What does it mean when a chemical reaction has an equilibrium constant of 173?
Mixture contains mostly products
400
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500
For the homogeneous gaseous reaction
A quantity of PCl5 was heated in a 1.0 L container at 250°C. At equilibrium, the gases were present in the following concentrations: PCl5 = 7.05 M, PCl3 = 0.54 M, Cl2 = 0.54 M. Calculate the value of the equilibrium constant for the dissociation of PCl5 at 250°C.
Keq = 0.041
500
What change would be expected to drive this reaction to the left?
NO2 (g) <--> 2NO2 (g)
An increase in pressure. This is due to how for every mole of reactant, there are 2 moles of product made.
500
N2(g)+3H2(g)⇌2NH3(g) ΔH=−92kJmol−1
What happened at t3?
Increase in Temperature
500
Consider the following reaction
A2(g) + B2(g) ⇋ 2AB(g)
If, at equilibrium, the concentrations are as follows: [A2] = 3.45 M, [B2] = 5.67 M and [AB] = 0.67 M
Find the value of the equilibrium constant, Keq
Keq = 0.023
500
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