# Equation Of Oxidation Chemistry: An Analysis Of Sodium Hypochlorate

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Introduction:

The purpose of this experiment is to determine the product that is produced from sodium hypochlorite oxidizing 2-ethyl-1,3-hexanediol and this experiment is to also determine if sodium hypochlorite is a selective oxidizing agent. This reaction is an oxidation reaction. The reaction involves the removal hydrogens and sometimes the addition of oxygen. 2-ethyl-1,3-hexanediol will undergo an oxidation reaction to produce an unknown product (Scheme 1). (1)

Scheme 1. 2-ethyl-1,3-hexanediol undergoes a reaction with sodium hypochlorite and glacial acetic acid to produce an unknown product.

There are three possible outcomes when 2-ethyl-1,3-hexanediol undergoes the oxidation reaction (Scheme 2, Scheme 3, and Scheme 4). (2)

Scheme 2. The first possible product when 2-ethyl-1,3-hexanediol undergoes

Calculation of moles of reactant.

The theoretical yield of the product was calculated by multiplying the mole of reagent by the mole of product. Exactly one mole of reagent would produce one mole of product (Equation 2).

( 0.00326 mol of 2-ethyl-1,3-hexanediol)/1 × (1 mol product)/(1 mol 2-ethyl-1,3-hexanediol) =0.00326 mol product for theortical yield of product (2)

Equation 2. Calculation of theoretical yield of product.

The mole of pure product was calculated by dividing the grams of product by the total gram found in one mole of 3-hydroxymethyl-4-heptanone (Equation 3).

(0.0545 g 3-hydroxymethyl-4-heptanone )/1 × (1 mol 3-hydroxymethyl-4-heptanone )/(144.23 g 3-hydroxymethyl-4-heptanone ) =0.00038 mol 3-hydroxymethyl-4-heptanone of pure product (3)

Equation 3. Calculation of mole of pure product.

Since 0.00326 mole of product was expected, dividing the actual yield of product by the expected yield would give the percent yield when it was multiplied by 100.

(0.00038 mol 3-hydroxymethyl-4-heptanone actual yield)/(0.00326 mol 3-hydroxymethyl-4-heptanone theortical yield) ×100 =11.656 % yield (4)

Equation 4. Calculation of percent

The purpose of this experiment is to determine the product that is produced from sodium hypochlorite oxidizing 2-ethyl-1,3-hexanediol and this experiment is to also determine if sodium hypochlorite is a selective oxidizing agent. This reaction is an oxidation reaction. The reaction involves the removal hydrogens and sometimes the addition of oxygen. 2-ethyl-1,3-hexanediol will undergo an oxidation reaction to produce an unknown product (Scheme 1). (1)

Scheme 1. 2-ethyl-1,3-hexanediol undergoes a reaction with sodium hypochlorite and glacial acetic acid to produce an unknown product.

There are three possible outcomes when 2-ethyl-1,3-hexanediol undergoes the oxidation reaction (Scheme 2, Scheme 3, and Scheme 4). (2)

Scheme 2. The first possible product when 2-ethyl-1,3-hexanediol undergoes

*…show more content…*Calculation of moles of reactant.

The theoretical yield of the product was calculated by multiplying the mole of reagent by the mole of product. Exactly one mole of reagent would produce one mole of product (Equation 2).

( 0.00326 mol of 2-ethyl-1,3-hexanediol)/1 × (1 mol product)/(1 mol 2-ethyl-1,3-hexanediol) =0.00326 mol product for theortical yield of product (2)

Equation 2. Calculation of theoretical yield of product.

The mole of pure product was calculated by dividing the grams of product by the total gram found in one mole of 3-hydroxymethyl-4-heptanone (Equation 3).

(0.0545 g 3-hydroxymethyl-4-heptanone )/1 × (1 mol 3-hydroxymethyl-4-heptanone )/(144.23 g 3-hydroxymethyl-4-heptanone ) =0.00038 mol 3-hydroxymethyl-4-heptanone of pure product (3)

Equation 3. Calculation of mole of pure product.

Since 0.00326 mole of product was expected, dividing the actual yield of product by the expected yield would give the percent yield when it was multiplied by 100.

(0.00038 mol 3-hydroxymethyl-4-heptanone actual yield)/(0.00326 mol 3-hydroxymethyl-4-heptanone theortical yield) ×100 =11.656 % yield (4)

Equation 4. Calculation of percent