University:
Massachusetts Institute of Technology
Course:
5.35 | Introduction to Experimental Chemistry
Academic year:

2022
Views:

118

Pages:

2
Author:

SparkyPet

Lab #3 Empirical Formula Copper Oxide The purpose of this lab was to synthesize Copper Oxide using 2 methods. First, we heat dry copper oxide powder until it fully reacts with oxygen from air to form copper oxide. For the second method we reacted an aqueous solution of copper (III) sulfate pentahydrate with sodium hydroxide to form copper (II) hydroxide. The empirical formula is useful because it can be used to determine the molecular formula of a compound. The molecular formula gives the actual number of atoms in one molecule of a compound. To determine the empirical formula of the compound formed when cooper combines with oxygen, is done by finding the number of moles of the elements in this case copper and oxygen in copper oxide and determining the simplest ratio between them. Data balanced equation for the copper oxide formation: 2Cu + O2 = 2CuO mass of empty beaker 35.000 g mass of beaker and copper 135.00 g (II) sulfate pentahydrate mass of empty test tube 25.000 g mass of test tube after 32.963 g heating and cooling 25.000 g - 32.963 = 7.963 7.963/ 249.68 = 0.032 mol 61 - 47.518 = 13.48 g of oxygen 13.48 g O x (1 mol O / 16.00 g O) = 0.843 mol The molar ratio between Cu and O is 1:1 According to molar ratio the Empirical Formula for Copper Oxide is: CuO

Experimental Chemistry Emperical Formula Copper Oxide

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