Question

if a chemical system at equilibrium is disturbed, the rates of the forward and reverse reactions are temporarily unequal. this is known as __________.
○ the law of mass action
○ the law of chemical equilibrium
○ the haber - bosch process
○ the unequal rate principle
○ le chateliers principle
question 7 (1 point)
which is not true regarding the effects temperature changes have on a system at chemical equilibrium?
○ a temperature increase favours the endothermic reaction.
○ a temperature decrease favours the exothermic reaction.
○ an increase in temperature increases $k_{eq}$ in an endothermic system.
○ an increase in temperature increases $k_{eq}$ in an exothermic system.
○ all of the above are true.
question 8 (1 point)
which change does not shift equilibrium toward reactant formation?
○ increasing product concentration
○ decreasing reactant concentration
○ decreasing product concentration
○ a and b
○ a, b, and c

Explanation:

Question 6

• The Law of Mass Action relates to reaction rates and equilibrium constants, not disturbance effects.
• The Law of Chemical Equilibrium defines the state of equilibrium, not disturbance response.
• The Haber - Bosch Process is a specific industrial process, not a principle about equilibrium disturbance.
• The Unequal Rate Principle is not a recognized principle for this concept.
• Le Chatelier's Principle states that if a chemical system at equilibrium is disturbed, the system will shift to counteract the disturbance, leading to temporary unequal forward and reverse reaction rates as it adjusts.

• A temperature increase favors the endothermic reaction (absorbs heat), so this is true.
• A temperature decrease favors the exothermic reaction (releases heat), so this is true.
• For an endothermic system, increasing temperature increases \(K_{eq}\) (more products formed), so this is true.
• For an exothermic system, increasing temperature decreases \(K_{eq}\) (since the reverse reaction, which is endothermic, is favored), so "An increase in temperature increases \(K_{eq}\) in an exothermic system" is not true.

• Increasing product concentration: According to Le Chatelier's Principle, the system will shift to consume products, so it shifts toward reactants.
• Decreasing reactant concentration: The system will shift to produce more reactants, so it shifts toward reactants.
• Decreasing product concentration: The system will shift to produce more products, so it shifts toward products (not reactants).
• Option a and b shift toward reactants, option c does not.

Answer:

E. Le Chatelier's Principle

Question 7