For a given equilibrium reaction for which #K_"eq"=6.4#...what scenario will alter the equilibrium value?

#"i. the use of a catalyst;"#
#"ii. an increase in the concentration of reactants;"#
#"iii. the equilibrium constant will remain unchanged;"#
#"iv. the use of a catalyst."#

Answer 1

Option #3#.

This is an easy question for someone who is informed. The equilibrium constant is CONSTANT, and does not depend on the concentrations of reactants and products. Obviously, if the concentrations of each reagent is changed, the direction of the equilibrium will move so as to satisfy the equilibrium. The equilibrium constant, however, remains constant at #6.4#.
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Answer 2

Any change in temperature, pressure, or concentrations of reactants or products will alter the equilibrium value of a reaction. Specifically, increasing the temperature will shift the equilibrium position in the direction of the endothermic reaction, while decreasing the temperature will favor the exothermic reaction. Similarly, changing the pressure (for reactions involving gases) or concentrations of reactants/products will cause the system to adjust to reach a new equilibrium position.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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