Question

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question 12 (1 point)
when the equilibrium constant is very small, the approximate concentration of
reactant at equilibrium is ______ the initial concentration.
○ greater than
○ less than
○ the same as
○ exactly 100 times
○ exactly 1 000 times
question 13 (1 point)
a reaction quotient is calculated to be 3.2 × 10⁻⁵. the equilibrium constant for the
same reaction is 5.4 × 10⁻⁵. which statement is correct?
○ the system is at equilibrium.
○ the concentrations of the products are greater than their concentrations at
equilibrium.
○ the system will attain equilibrium by moving to the right.
○ the system will attain equilibrium by moving to the left.
○ the rate of the forward and reverse reactions are different at equilibrium.
question 14 (1 point)
hydrogen is the lightest of elements with atomic number one. when hydrogen gas
reacts with bromine gas, they form hydrogen bromide gas, i.e., h₂(g) +
br₂(g) ⇌ 2hbr(g)
at equilibrium, concentration values of the compounds are:
table with compound, h₂(g), br₂(g), hbr(g) and equilibrium concentrations: 0.024 mol/l, 0.024 mol/l, 0.08 mol/l (partially visible)

Explanation:

Question 12

When the equilibrium constant \(K\) is very small (\(K=\frac{[products]}{[reactants]}\)), it means that the reaction does not proceed much in the forward direction. So, most of the reactant remains unreacted. Thus, the approximate concentration of reactant at equilibrium is the same as the initial concentration.

We know that if \(Q = K\), the system is at equilibrium. If \(Q K\), the reaction will shift to the left (towards reactants) to reach equilibrium. Here, \(Q = 3.2\times10^{-5}\) and \(K=5.4\times 10^{-5}\), so \(Q

Answer:

the same as

Question 13