Investigation 6: The Copper Cycle
CHEM 101 Lab-M/630
As an investigation of the copper cycle lab group 6 conducted an experiment on 6 October 2014 at Arizona State University laboratory that would demonstrate the cycle of reactions that copper (Cu) can produce when introduced to with other substances/reactant. The purpose of the investigation was to notice the transformation of a specific quantity of copper wire (g) as it undergoes its coordination reactions until a reduction method would yield copper (Cu) again. The final regeneration of copper (Cu) was then weighed to present a percent recovery of the copper (Cu) as it cycled through its series of reactions. To present an effective experiment the following equipment: copper wire, hot plate, 3M HCl(aq), 6M HNO3(aq), 6M NaOH (aq), 2 M H2SO4, 100ml beaker, graduated cylinder, filter flask, Buchner funnel/vacuum flask , scale, and pipets alongside the fume hood--for the omission of NO2-- was used to conduct the copper cycle experiment. First, the given copper wire (.29g) was cut into minute pieces then placed in a beaker with the aqueous solution of HNO3. The beaker was then placed on the hot plate to present a blue transparent homogenous mixture of Copper (II) Nitrate(aq)—Cu(NO3)2(aq). The reaction of copper and HNO3 was oxidative due to a gas being produced within the reaction. Secondly, lab group 6 took the Copper (II) Nitrate and slowly added 125 drops of NaOH by way of a pipet. Lab group 6 noticed solid blue crystals begin to form almost immediately, thus presenting a precipitate (s) and the compound Copper Hydroxide(s)—Cu(OH)2. For the third reaction, 90 drops of H2SO4 from the pipet was introduced to the Copper Hydroxide(s) to create an acid/base neutral reaction to form Copper Sulfate(aq)—CuSO4(aq). Fourthly, lab group 6 slowly added granules of Zinc (Zn) to the Copper Sulfate until the reduction method took place and therefore produced metallic copper(s) within the beaker. The excess...
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