Equilibrium

K>1; The reaction favors forming products over reactants

K<<1; The reaction greatly favors forming reactants over products.

K>>1; The reaction greatly favors forming products over reactants

K<; The reaction greatly favors reactants over products

They apply to concentrations in expression for K.

They determine which side is favored at equilibrium.

They indicate how many trials must be conducted to determine K accurately.

They become subscripts in the chemical formulae involved in K.

The system rapidly achieves equilibrium due to favorable kinetics despite low product formation.

The system has mostly reactants present at equilibrium.

We cannot determine anything about product or reactant predominance from K alone without rate data.

The system has exclusively products present at equilibrium with no reactants left.

There are equal concentrations of reactants and products at equilibrium.

Products are favored over reactants.

Neither reactants nor products are favored.

Reactants are favored over products.

The larger the equilibrium constant, the more complete the reaction at equilibrium.

There is no relation between the size of K and the extent of reaction.

A small equilibrium constant indicates an increase in product concentration.

The larger the equilibrium constant, the less complete the reaction at equilibrium.

The rate of the forward reaction must be necessarily slower for the reaction with the smaller K at lower pressures or more information must be available to determine the cause of its weakness compared to the other reaction with a higher K value under proper temperature conditions.

A specific reaction with a smaller equilibrium constant tends to form less of its products at relative to reactants at higher temperatures.

There is an equal propensity for both forward and reverse reactions under standard conditions.

The reaction proceeds hardly at all in the forward direction under standard conditions.

Only dynamic equilibrium can be established but not static equilibrium under standard conditions.

The reaction goes quickly to completion in the forward direction under standard conditions.

It increases only product concentrations without shifting position.

It shifts the position toward the reactants.

There is no effect on either product or reactant concentrations.

It shifts the position toward the products.

10^10

10^-4

10^0

10^2

The rate constants for forward and reverse reactions are equal.

The reactants are favored over products at equilibrium.

The products decompose into reactants spontaneously.

No reaction occurs because K is too low to proceed with any reactions.