AP Chem- Equilibrium

What is dynamic equilibrium?

Dynamic equilibrium in a chemical reaction is the condition in which the rate of the forward reaction equals the rate of the reverse reaction.

Why is it called dynamic?

Dynamic equilibrium is called dynamic because the forward and reverse reactions are still occurring, however, they are occurring at the same rate.

Express the equilibrium constant for the combustion of propane: C3H8(g)+5O2(g)⇌3CO2(g)+4H2O(g)

K=[CO2]3[H2O]4/[C3H8][O2]5

What is the correct expression for the equilibrium constant (Kc)(Kc) for the reaction between carbon and hydrogen gas to form methane shown here? C(s)+2H2(g)⇌CH4(g)

Kc=[CH4]/[H2]2

For the reaction 2A(g)⇌B(g)2A(g)⇌B(g), the equilibrium constant is KpKp = 2.0. A reaction mixture initially contains 10.0 atmatm of gas (PAPA=2.0 atmatm and PBPB = 8.0 atmatm).

The reaction mixture is at equilibrium.

If a reaction is exothermic and produces large quantities of heat reaching equilibrium, its equilibrium constant will be

greater than zero.

A reaction that has a large equilibrium constant has

more products then reactants at equilibrium.

Consider the reaction N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) where N2O4N2O4 is colorless and NO2NO2 is brown. At a temperature of 5∘C∘C, the reaction is colorless at equilibrium. This indicates that the equilibrium constant for this reaction at this temperature is

small (less than 1).

A chemical reaction is at equilibrium when

the rate of the forward reaction equals the rate of the reverse reaction.