5. A chemist mixes 5.216 g of potassium permanganate, 2.318 g of ethanol, and ex

Question

5. A chemist mixes 5.216 g of potassium permanganate, 2.318 g of ethanol, and excess sulfuric acid. These chemicals react as follows: Please repor rt all of your answers for this problem to the correct number of significant figures. C. What mass of acetic acid is produced in this reaction assuming that the reaction goes to completion? ethanol) are left over? mass of sulfuric acid is consumed in this reaction, assuming that the reaction goes to completion? te the percent yield of acetic acid in this experiment. he reaction went to completion. How many grams of excess reactant (either potassium permanganate or

Explanation / Answer

moles of potassium permagnet= 5.216g/158gmol-1 =0.033mol

moles of ethanol=2.318g/46gmol-1= 0.050mol

As we can see here the limiting agent is potassium permagnate because for whole consumption only 0.041 mol ethanol required and we have ethanol 0.05 mol.

a.) moles of H2SO4 required= moles of potassium permaganet x 6 /4

= 0.033 x 6/4 = 0.0495 mol

b.) theoretical yield of CH3COOH= moles of potassium permagnet x 5 /4

= 0.033 x 5/4 = 0.04125 mol

mass produce = mol x molar mass

= 0.04125 x 60

= 2.475 g

percent yield= (actual yield/ theoretical yield ) x 100

= (1.697/ 2.475) x 100

= 68.56 %

c.) mass of acetic acid produced when reaction get completed is calculated above that is theoretical yield

=moles of potassium permagnet x 5 /4

= 0.033 x 5/4 = 0.04125 mol

mass produce = mol x molar mass

= 0.04125 x 60

= 2.475 g

d.) excess reactant is ethanol. that is,

0.05 - 0.033 x 5/4 = 0.00875 mol.

mass = 0.00875 x 46 = 0.4025 g

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