The reaction 2 NO(g) ⇌ N2(g) + O2(g) has a value of Keq = 2400 at a temperature of 2000 K. If 0.570 mol of NO(g) is initially placed in a 3.0 L container, calculate the equilibrium concentrations of each gas

Explanation:

Hello,

In this case, for the given chemical reaction, we write the following law of mass action:

That in terms of the change due to the reaction extent (ICE procedure) we can write:

Thus, the initial concentration of nitrogen monoxide is:

Thereby, we write:

That we can solve by suing the quadratic equation formula or solver to obtain two roots:

Nevertheless, the correct answer is 0.094 M since the other root will produce a negative concentration of nitrogen monoxide at equilibrium, therefore, the equilibrium concentrations turn out:

Best regards.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.