For each of the following equilibria, write the equilibrium constant expression for Kc. Where appropriate, also write the equilibrium constant expression for Kp. WO3(s)+3H2(g)?W(s)+3H2O(g)

a. Kc=[H2]3[H2O]3
b. Kc=[H2O]3[W][H2]3[WO3]
c. Kc=[H2O]3[H2]3
d. Kc=[H2]3[WO3][H2O]3[W]

Answer in explanation

Explanation:

The question asks to write the equilibrium constant expression for the equation. This can be written by placing each of the products in square brackets and raise them to their number of moles, divided by the reactants each raised too, based on number of moles.

The square brackets represent the concentration of the compounds. We write the equilibrium constant expression as follows:

Kc = [H2O]^3[W]/[H2]^3[WO3]

For the equilibrium constant in terms of pressure, we use only the reactants and products that are gaseous.

Kp = [H2O]^3/[H2]^3

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.

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.