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Chemical Risk Precautions Lab Report

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1. Risk Assessment Chemical Risk Precautions Fe(nail) Low glasses, lab coats, gloves Cu(plate) Low glasses, lab coats, gloves Zn(powder) Highly flammable keep away from open fire, wear glasses, lab coats, gloves KNO3(aq) Low glasses, lab coats, gloves FeSO4(aq) Harmful if swallowed glasses, lab coats, gloves, avoid swallowing CuSO4(aq) Harmful if swallowed glasses, lab coats, gloves, avoid swallowing ZnSO4(aq) Harmful if swallowed glasses, lab coats, gloves, avoid swallowing 2. Introduction An electrochemical cell is an energy source that generate the potential difference between electrodes using redox reactions. Oxidation-reduction reactions are used to ensure e.m.f. in the electrochemical cells. The electromotive force (ε) is the output energy provided by a cell and it is measured in volts (V). The value of e.m.f. …show more content…

Discussion 1) A balanced chemical reaction: Zn + CuSO4 ZnSO4 + Cu A full ionic reaction: Zn0(s) + Cu2+(aq) + SO42-(aq) Zn2+(aq) + SO42-(aq) + Cu0(s) A net ionic reaction: Zn0(s) + Cu2+(aq) Zn2+(aq) + Cu0(s) Cu2+ + 2e Cu0 - is an oxidant, reduced Zn2+ Zn0 + 2e- - is a reductant, oxidized 2) An iron/zinc cell (Exp.3): On the cathode (+ve): Fe2+(aq) +2e- Fe0(s) - is an oxidant, reduced On the anode (-ve):Zn0(s) Zn2+ (aq) + 2e- - is a reductant, oxidized In the Exp.3 the voltage of the iron electrode (Fe2+) is greater than voltage of zinc electrode (Zn2+): E0 (Zn2+) =-0.763 V and E0 (Fe2+) =-0.44 V. Due to this fact, the iron electrode reacts as an oxidant and it reduced on the cathode. An iron/copper cell (Exp.4): On the cathode (+ve): Cu2+(aq) + 2e Cu0(s) - is an oxidant, reduced On the anode (-ve): Fe0(s) Fe2+(aq) +2e- - is a reductant, oxidized In the Exp.4, the values of the voltage for iron and copper are E0 (Fe2+) =-0.44 V and E0 (Cu2+)=+0.337 V respectively. In this case, the iron reacted such as a reductant and it oxidized on the

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An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

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