According to the Law of Conservation of Mass, the mass of the products must equal the mass of the reactants, so logically one would expect that if 2 g of copper was used to start the lab, the lab would result in 2 g of copper.
In this lab, each group had the initial mass of the copper close to 2.00 grams. Post-Lab Report (a) Report the collected data with the correct uncertainty. Show one sample calculation trial 1 trial 2 trial 3 mass copper chloride (c) Calculate the mass of chlorine. The result of this copper lab should have been that the mass of the initial copper and the mass of the final copper equals each other.
trial initial volume final volume (mL) concentration mass copper (&/L) 16. ol a O: 95% (b) Calculate the mass of copper chloride in the volume of solution used. Unfortunately, that was not the case in this lab, and the final mass of copper exceeded the initial mass by 4.841g. Reagent Appearance Volume or Mass Concentration H2SO4 (aq) Clear and 15 mL 1.5 M Transparent Zn (s) (dust) Grey in color 0.15 g N/A Ethanol Clear and 5 mL N/A transparent solution The blue green ammonia complex is reacted with 15 mL of 1.5 M H2SO4 to make another complex, and then it is reacted to 0.15 g of Zn dust to obtain elemental Copper metal.
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