The value of δh° for the reaction below is -126 kj. the amount of heat that is released by the reaction of 10.0 g of na2o2 with water is kj. 2na2o2 (s) + 2h2o (l) → 4naoh (s) + o2 (g)

The enthalpy of the reaction for given amount of will be -8.064 kJ.

Explanation:

To calculate the number of moles, we use the equation:

Given mass of = 10 g

Molar mass of = 78 g/mol

Putting values in above equation, we get:

For the given chemical reaction:

By Stoichiometry of the reaction:

If 2 moles of produces -126 kJ of energy.

Then, 0.128 moles of will produce = of energy.

Thus, the enthalpy of the reaction for given amount of will be -8.064 kJ.

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.