Experimental Chemistry Emperical Formula Copper Oxide. PDF

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This is a Laboratory Report for Experimental Chemistry 111...

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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 mass of beaker and copper (II) sulfate pentahydrate mass of empty test tube mass of test tube after 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

35.000 g 135.00 g

25.000 g 32.963 g

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...