The following reactions have the indicated equilibrium constants at a particular temperature: n2(g) + o2(g) ⇌ 2no(g) kc = 4.3 × 10−25 2no(g) + o2(g) ⇌ 2no2(g) kc = 6.4 × 109 determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4no(g) ⇌ n2(g) + 2no2(g)

Explanation:

We have the reactions:

A:

B:

Our target reaction is:

We have as a reactive in the target reaction and   is present in A reaction but in the products side. So we have to flip reaction A.

A:

Then if we add reactions A and B we can obtain the target reaction, so:

A:

B:

For the final Kc value, we have to keep in mind that when we have to add chemical reactions the total Kc value would be the multiplication of the Kc values in the previous reactions.

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.

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.