Question

question 5 (1 point)
in the equilibrium constant expression below, what do the exponents represent?
$k_{eq} = \frac{c^cd^d}{a^ab^b}$
\bigcirc the concentrations of reactants and products
\bigcirc the equilibrium constant
\bigcirc the rates of the forward and reverse reactions
\bigcirc the stoichiometric coefficients from the balanced equation
\bigcirc none of these

question 6 (1 point)
what does it mean if $k_{eq} < 1$, at equilibrium?
\bigcirc the concentration of reactants is greater than the concentration of products.
\bigcirc the concentration of products is greater than the concentration of reactants.
\bigcirc the rate of the forward reaction is greater than the rate of the reverse reaction.
\bigcirc the rate of the reverse reaction is greater than the rate of the forward reaction.
\bigcirc the concentration of products and reactants are about the same.

question 7 (1 point)
when pressure \underline{\hspace{0.5cm}i\hspace{0.5cm}} and volume \underline{\hspace{0.5cm}ii\hspace{0.5cm}}, the reaction in an equilibrium system shifts in
the direction that produces \underline{\hspace{0.5cm}iii\hspace{0.5cm}} particles.
the statement given above is completed by the information given in the row:

Explanation:

Question 5

In the equilibrium constant expression \(K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b}\), the exponents \(a\), \(b\), \(c\), and \(d\) are derived from the balanced chemical equation. For a general reaction \(aA + bB
ightleftharpoons cC + dD\), these exponents represent the stoichiometric coefficients of the reactants (\(A\) and \(B\)) and products (\(C\) and \(D\)). The concentrations of reactants and products are represented by the terms inside the brackets (\([A]\), \([B]\), \([C]\), \([D]\)). The equilibrium constant is \(K_{eq}\) itself. The rates of the forward and reverse reactions are related to the rate - law expressions (not directly to the exponents in the equilibrium constant expression).

The equilibrium constant \(K_{eq}=\frac{[products]}{[reactants]}\). If \(K_{eq}<1\), then \(\frac{[products]}{[reactants]}<1\), which implies \([reactants]>[products]\). The equilibrium constant is related to the concentrations of reactants and products at equilibrium, not directly to the rates of the forward and reverse reactions (although at equilibrium, the rate of the forward reaction equals the rate of the reverse reaction). When \(K_{eq}\approx1\), the concentrations of products and reactants are about the same.

Answer:

the stoichiometric coefficients from the balanced equation

Question 6