Of the following equilibria, only will shift to the left in response to a decrease in volume. a) 4 fe (s) 3 o2 (g) 2 fe2o3 (s) b) h2 (g) cl2 (g) 2 hcl (g) c) 2hi (g) h2 (g) i2 (g) d) 2 so3 (g) 2 so2 (g) o2 (g) e) n2 (g) 3 h2 (g) 2 nh3 (g)

D

Explanation:

The direction of the reaction by changing the concentration can be determined by Le Chatelier's principle,  

It states that ,  

When a reaction is at equilibrium , Changing the concentration , pressure,  temperature disturbs the equilibrium , and the reaction again tries to attain equilibrium by counteracting the change.

According to Le Chatelier's principle,

If the pressure is increased , the equilibrium of the reaction is disturbed , so, the reaction will move in order to decrease the pressure.

The molecules of gas are responsible for pressure ,  So,  To decrease the pressure reaction will go towards the side with less number of gaseous molecules.

Effect of change in volume -

Pressure and volume of the system are inversely proportional to each other. So if the volume of the system is decreased, the pressure of the system will increase and hence, equilibrium of the system will be disturbed. In order to attain equilibrium again, system will move towards the side having less no. of gaseous molecules to decrease pressure.

A)

Gaseous molecules on right side = 0

Gaseous molecules on left side = 1

Gaseous molecules on right side  < Gaseous molecules on left side, the equilibrium will shift right.

B)

Gaseous molecules on right side = 2

Gaseous molecules on left side = 2

Gaseous molecules on right side  = Gaseous molecules on left side, the equilibrium will not be attained.

C)

Gaseous molecules on right side = 2

Gaseous molecules on left side = 2

Gaseous molecules on right side  = Gaseous molecules on left side, the equilibrium will not be attained.

D)

Gaseous molecules on right side = 3

Gaseous molecules on left side = 2

Gaseous molecules on right side  > Gaseous molecules on left side, the equilibrium will shift left.

E)

Gaseous molecules on right side = 2

Gaseous molecules on left side = 4

Gaseous molecules on right side  < Gaseous molecules on left side, the equilibrium will shift right.

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.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: