Experiment 9/5 Voltaic cells AIM How the change the concentration of the electrolyte CuSo4 (solution of ions) affect the voltage of the electrochemical cell BACKGROUND An electrochemical cell is also called a voltaic cell‚ which derives electrical energy from redox reaction taking place within the cell. It consists of two different metals that are connected by a salt bridge. Eletrons always flow from anode to cathode‚ where anode is negative (reduction) and cathode is positive (oxidation)
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buildings could very well be rusting and dissolving around us. Metal/ Cation or Solution HCl H2O CuSO4 ZnSO4 MgSO4 SnCl2 Fe(NO3)3 Cu NR NR NR NR NR NR NR Mg R NR R R NR R R Sn R NR R NR NR NR NR Zn R NR R NR NR R R Fe R NR R NR NR R NR Steel (FeAl) R NR R NR NR R NR Table 1 : Predictions Metal/Cation Or Solution HCL Mg2+ H2O Cu2+ Zn2+ Fe2+ Sn2+ Cu Rusted‚ Less shiny No reaction No reaction bubbles bubbles tarnished No reaction Mg Bubbles‚ Hydrogen
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negative terminal electrolyte‚ the higher the potential difference in voltaic cell. Variables: Manipulated variable | Concentration of negative terminal electrolyte * Use zinc sulphate solution‚ ZnSO4 as the negative terminal electrolyte throughout the experiment * Use zinc sulphate solution‚ ZnSO4 of different concentration‚ 1.0M‚ 0.10M‚ 0.010M and 0.0010M
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Katerina Baeza Hernandez | | | | | | | |Zn |Mg |Cu |Pb | | |(+) clear liquid but the |(+) a black spot appeared on|(-) no reaction occurred |(-) no reaction | |Pb(NO3)2
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TITLE : The copper cycle IN TRODUCTION The purpose of the experiment is to recognize that change of state‚ change in colour‚ formation of a precipitate‚ or the evolution of heat are associated with a chemical change; to study reactions of copper. Copper is an element that can be found in nature in a variety of different compounds. The most common natural ore is the sulphide‚ known as chalcocite‚ Cu2S. This mineral is an important source of copper metal because it is about 80% copper by
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experimental method produces more accurate result. One was electrochemistry using a Daniel cell and the other one was spectrometry by estimating concentration of complex solution using a calibration curve. The formation constant of cupric ammine complex Cu(NH3)42+‚ Kf‚ came out with 1.93x10^15 using electrochemical cell method and 9.79x10^12 using spectrophotometer method. Considering the literature value of Kf is around 4.8x10^12 ~ 1.7x10^13‚ spectrophotometer gives more accurate result than electrochemical
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Copper Sulphate solution (CuSO4) in a measuring cylinder‚ for precise accuracy‚ and then pour the solution into test tube. I will place the test tube into a beaker and insulate the test tube‚ for minimum heat loss. (As shown in the diagram above.) 2.Secondly I will measure the required amount of Zinc (Zn) on a weighing scale‚ again for precise accuracy. I will then measure the starting temperature using a thermometer. Next I will pour the Zinc into the test tube containing CuSO4. 3.Finally I will measure
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single-displacement reaction. Here are the chemical formulas of the reactants for each reaction: • zinc – Zn copper sulfate – CuSO4 In well 1A there was a chemical reaction which turned the zinc black‚ while the copper sulfate was still blue. AX + B → A + BX Zn + CuSO4 → ZnSO4 +Cu • aluminum – Al copper sulfate – CuSO4 In well 2A there was no reaction between the aluminum and copper sulfate. The aluminum floated and there was no
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es. The enthalpy and entropy changes of a system undergoing such processes are interrelated by the change in free energy‚ ªG‚ according to the equation ªG = ªH - T ªS (1) This investigation focuses on the reaction Zn(S ) + CuSO4(aq) Y ZnSO4(aq) + Cu(S ) (2) ªG will be calculated from the ªH and ªS values obtained electrochemically. The validity of Equation (1) will be tested by comparing the value of ªH obtained electrochemically with the value of ªH obtained calorimetrically
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with 0.10M Cu+2 solution. E˚ for copper electrode is 0.34V. 2. Calculate EMF of the cell involving the reaction : Mg(s)+ 2Ag+(aq) → Mg+2(aq) + 2Ag(s) Given; [Mg+2] = 0.130M and [Ag+] = 1.0x10-4M & E˚Ag+/Ag = 0.80V and E˚Mg+2/Mg = -2.37V. 3. Calculate the EMF of the cell: Zn│Zn+2(1M)║ Ag+(1M)│Ag ; Given; E˚Zn/Zn+2 = 0.762V
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