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

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.