An equilibrium mixture of N2, O2and NO gases at 1500K is determined to consist of 6.4 x 10-3Mof N2, 1.7 x 10-3M O2, and 1.1 x 10-5M NO. Write the equilibrium expression and solve for the equilibrium constant (Keq) for the systemat this temperature?

Explanation:

consist of 6.4 x 10-3Mof N2, 1.7 x 10-3M O2, and 1.1 x 10-5M NO. Write the equilibrium expression and solve for the equilibrium constant (Keq) for the systemat this temperature?

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.

the volume increases