Alum is a compound used in a variety of applications including cosmetics, water purification, and as a food additive. it can be synthesized from aluminum metal, sulfuric acid, water, and potassium hydroxide, as seen in the equation. 2 al(s) 2 koh(aq) 4 h2so4(aq) 10 h2o(l) ⟶ 2 kal(so4)2∙12 h2o(s) 3 h2(g) alum using the data, determine the theoretical and percent yield for this alum synthesis. note that aluminum is the limiting reactant. description mass (g) bottle mass 10.221 bottle mass with aluminum pieces 11.353 final product and bottle mass 19.230 what is the theoretical yield of alum

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

Explanation:

Mass of bottle = 10.221 g

Mass of bottle with aluminium pieces = 11.353 g

Mass of aluminium = 11.353 g - 10.221 g = 1.132 g

Mass of alum and bottle = 19.230 g

Mass of alum =  19.230 g - 10.221 g = 9.009 g

Experimental yield of alum =  9.009 g

Theoretical yield of alum:

Moles of aluminium =

According to reaction, 2 moles of aluminum gives 2 moles of alum.

Then 0.041926 mol aluminium will give :

of alum.

Mass of 0.041926 moles of alum:

0.041926 mol × 474 g/mol= 19.873 g

Theoretical yield of alum = 19.873 g

Percentage yield:

Percentage yield of the alum:

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

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.

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