Chemical Equilibrium Quiz & Flashcards

Chemical equilibrium is reached when concentrations remain constant, not necessarily equal.

A K value much less than 1 indicates the reaction favors reactants.

A catalyst speeds up the attainment of equilibrium without changing its position.

Decreasing pressure shifts equilibrium to the side with more moles of gas.

Only temperature affects the value of K; catalysts and other factors do not.

Exothermic reactions shift towards products when temperature decreases.

Reversing a reaction inverts the equilibrium constant.

Adding a reactant shifts equilibrium towards products (right).

Removing a product shifts the equilibrium to form more products.

Increasing temperature favors the endothermic direction, shifting right.

For exothermic reactions, increasing temperature decreases K.

Pressure changes do not affect equilibrium if the moles of gas are equal on both sides.

Dynamic equilibrium occurs when forward and reverse reaction rates are equal.

Decreasing a reactant's concentration shifts equilibrium towards reactants (left).

Q = K indicates the system is at equilibrium.

All listed actions will shift equilibrium to the left.

Adding an inert gas at constant volume does not affect equilibrium.

For gases, the equilibrium constant is expressed in terms of partial pressures (Kp).

Adding solvent dilutes concentrations, which can shift equilibrium if reactants or products are affected.

Increasing pressure shifts equilibrium towards the side with fewer moles of gas.

For endothermic reactions, the equilibrium constant increases with temperature.

Catalysts speed up both reactions equally, leaving the equilibrium constant unchanged.

Increasing temperature shifts exothermic reactions to the left, favoring reactants.

At equilibrium, the free energy change is zero, indicating no net change.

When reactions are combined, their equilibrium constants are multiplied.

A misconception is that equilibrium means equal concentrations, which is not true.

Increasing product concentration shifts equilibrium towards reactants (left).

The equilibrium constant is only affected by temperature changes.

Heating an endothermic reaction shifts equilibrium to the right, favoring products.

A large K indicates that products are favored at equilibrium.

Decreasing temperature favors the exothermic direction, shifting right.

Adding a product shifts equilibrium towards reactants (left).

At equilibrium, the rates of the forward and reverse reactions are equal.

Equilibrium is dynamic because reactions continue with no net change in concentrations.

Removing a reactant shifts equilibrium towards reactants (left).

Equilibrium determines the extent of reactant conversion in reversible reactions.

At equilibrium, no net change in concentrations occurs, though reactions continue.

Increasing pressure shifts equilibrium towards the side with fewer moles of gas.

Increasing pressure shifts equilibrium towards the side with fewer moles of gas.

A small equilibrium constant means reactants are favored at equilibrium.

Altering stoichiometry changes the equilibrium constant as it depends on stoichiometric coefficients.

The equilibrium expression is products over reactants, each raised to the power of their coefficients.

If Q > K, the reaction shifts towards reactants to reach equilibrium.

Doubling coefficients results in squaring the equilibrium constant.

Dynamic equilibrium is reached when forward and reverse reaction rates are equal.

Increasing temperature in an endothermic reaction shifts equilibrium to the right.

Decreasing temperature in an exothermic reaction shifts equilibrium to the right.

ΔG = 0 indicates the system is at equilibrium, with no net change occurring.

All listed conditions favor product formation by shifting equilibrium to the right.