Consider the reaction below.

2 upper N subscript 2 upper O subscript 5 (g) double-headed arrow 4 upper N upper O subscript 2 (g) plus upper o subscript 2 (g).

If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?

The forward and reverse reactions no longer occur.

The rates of the forward and reverse reactions are unequal.

The concentrations of the products and reactants do not change.

The forward reaction stops at 500 K.

The concentrations of the products and reactants do not change

Explanation:

A system is said to be in equilibrium when there is no observable change in concentration of the reactants and products with time.

However, a dynamic equilibrium occurs when the rate of the forward and backward reaction are the same. This implies that the concentration of the reactants and products do not change as long as the physical state of the system is kept constant.

the answer is:  

line graphs show patterns in data with variables that change over time; whereas, circle graphs show data as parts out of a whole (such as out of 100%).