1) Complete the table to show what would happen to the position of the following gas phase equilibria if the following changes were made. Tick the correct column in each case.
Equilibrium
Energy Increase temperature
Increase pressure
change
moves
moves
move
(forward left
right left
right
reaction)
Ale) + 2 B(g) = X(g) + Zig) exothermic
endothermic
Ple) + Qig) = 2 Xig)
exothermic
A2(g) = X(g) + 2(g)
endothermic
2 Pig) = 2 C(s) + D(g)

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.

1.solid

2.carbon dioxide

3.helium

you didnt put any of the following