Consider the following equilibrium:

4fe(s) + 3 o2(g) < -- --> 2fe2o3(s);

which of the following equations is wrong?
kp=kc(rt)-5
kc=[o2]-3
kp= kc(rt)-3
kp = po2-3

The equation which is wrong is

Explanation:

For the given reaction:

The expression for is given by:

The concentration of solids are taken to be 1, only concentration of gases and liquid states are taken. The pressure of only gases are taken.

Relationship between is given by the expression:

where,

= number of moles of gaseous products - number of moles of gaseous reactants

R = gas constant

T= temperature

For the above reaction,

= number of moles of gaseous products - number of moles of gaseous reactants = 0 - 3 = -3

Hence, the expression for is:

Therefore, the equation which is wrong is

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

you need to give more information