Question

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question 9 (1 point)
which of these affects the equilibrium constant, $k_{eq}$?
\bigcirc concentration
\bigcirc pressure
\bigcirc volume
\bigcirc temperature
\bigcirc all of the above

question 10 (1 point)
when the temperature \underline{i} in a system in which the forward reaction is \underline{ii},
equilibrium shifts toward \underline{iii} formation.
the statement given above is completed by the information given in the row:

row	i	ii	iii
b	increases	exothermic	product
c	increases	endothermic	reactant
d	decreases	endothermic	product
e	decreases	exothermic	reactant

\bigcirc a
\bigcirc b
\bigcirc c
\bigcirc d
\bigcirc e

question 11 (1 point)

Explanation:

Question 9

The equilibrium constant \(K_{eq}\) is only affected by temperature. Changes in concentration, pressure, or volume shift the equilibrium position (using Le - Chatelier's principle) but do not change the value of \(K_{eq}\).

• For an endothermic reaction (\(\Delta H> 0\)), heat is a reactant. When the temperature (i) increases, according to Le - Chatelier's principle, the system will shift to consume the added heat. For an endothermic forward reaction, increasing the temperature (i = increases) will shift the equilibrium towards the product (iii) side (because the forward reaction absorbs the added heat).
• If the reaction is exothermic (\(\Delta H<0\)), heat is a product. Increasing the temperature would shift the equilibrium towards the reactant side, and decreasing the temperature would shift it towards the product side.

Answer:

temperature

Question 10