inadvertently produce undesired products that must be filtered or decanted out of solution (Petrucci et al‚ 2007). Beginning with pure copper wire‚ this experiment will exhibit its transformation to substances including Cu(NO3)2‚ Cu(OH)2‚ CuO‚ CuSO4 . 5H2O and finally returning to pure copper (Cu). The experiment objective is to successfully complete these conversions and then calculate the percentage of recovered copper using the initial and final mass data obtained. Procedure Please refer to "Experiment
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-----> 2HBr 2. Potassium Chlorate ----> Potassium Chloride + Oxygen = KClO3 ------> KCl + O2 KClO3 ------> KCl + O2 Balanced = 2KClO3 ------> 2KCl + 3O2 3. FeCl3 + 3NaOH = Fe(OH)3 + 3NaCl 4. Zn (s) + H2SO4 (aq) = ZnSO4 (aq) + H2 (g) 5. CuS + HNO3 -> CuSO4 + H2O + N2O CuS + 2 HNO3 -> CuSO4 + H2O + N2O Chemical Reaction is a process that involves rearrangement of the molecular or ionic structure of a substance‚ as opposed to a change in physical form or a nuclear reaction. Reactant
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ONE-SCHOOL.NET Short Notes: Form 5 Chemistry Rate or Reaction Calculation Rate of Reaction (Average Rate) Rates of reaction = Quantity change of reactants/products Total time for the reaction If the quantity change is immeasurable Rates of reaction = 1 Total time for the reaction Find the Rate From a Graph Average Rate Rates At an Instant The rate of reaction is equal to the slope of the graph The rate of reaction at an instant‚ t‚ is equal to the of quantity against
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be used to produce electricity and electricity can be used to cause chemical reactions through oxidation-reduction reactions. The first part of the experiment measures the standard electrode potentials of five various half cells against the Cu2+(1M)|Cu half cell. The last three half cells are prepared through electrolysis. The electrode potentials of all reactions are positive which means that they are spontaneous. There is a significant percent difference from the theoretical and the experimental
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Zn(s) + CuSO4(aq) ------ Cu(s) + ZnSO4 (aq) The enthalpy changees for two different reactions will be determined practically. In the first‚ experiment delta H will be determined directly and account will be taken of heat losses by extrapolation of an appropriate graph. The second experiment involves teh inderect determination of an enthalpy change using Hess’ Law. The temperature can be measured manually but this experiment is ideal for using a data logger. In the first experiment we are trying
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Determining an Enthalapy Change of Reaction Purpose of Experiment The purpose of this experiment is to determine the enthalapy change for the displacement reaction: Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq) Hypothesis With this experiment I can also not make a hypothesis‚ because we did actually not do the experiment‚ but we were told that the temperature would make a sudden drop ‚ but we can measure the ΔT of the surrounding. The reaction is endothermic because the system will take in energy
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Oxidation and Reduction Mnemonic: OILRIG Oxidation Is Loss‚ Reduction Is Gain Oxidation → the loss of electrons from an atom or an ion→ always happens at anode (positive electrode) → think anOde (O2 in the electrolysis of water xp) Redox reactions: Reactions involving the transfer of electrons e.g. burning‚ rusting‚ photosynthesis‚ respiration and the browning of apples. happens in three types of reactions: 1. addition of oxygen 2. removal of hydrogen 3. increase in valency (how easily an atom
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Determine the enthalpy change for the reaction (ΔHfθ) between zinc and copper sulphate solution‚ giving full practical details. Aim To determine the enthalpy change for the reaction between zinc and copper sulphate. Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s) Introduction In the study of energy (thermodynamics) the system refers to the reacting chemicals (zinc and copper sulphate solution) and the surroundings is everything else (atmosphere‚ container‚ temperature probe). By
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aqueous sodium sulphate and water. 2. Balance the following equation. a. Fe(s)+CuSo4 (aq)---(FeSo4(aq)+Cu(s) b.H2So2(aq)+NaOH(aq)-(Na2SO4(aq)+H2O(l) c.Ba(OH)2(aq)+HBr(aq)-(BaBr2(aq)+H 2O(l) 3.What is differences between combination and decomposition reaction? Explain with examples. 4. Can a displacement reaction be a redox reaction? Explain with examples. 5.Complete and balance a. Cu+AgNO3--(
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off to the surroundings; thus‚ temperature of the surroundings will increase. By measuring the change in the temperature and using the formula Q= mcΔT‚ we can calculate the enthalpy change of the reaction. Equation 1: CuSO4 + Zn ZnSO4 Ionic Equation: Zn (s) + Cu2+ (aq) Cu (s) + Zn2+ (aq) MATERIALS/APPARATUS: * 1 insulated Styrofoam cup * Copper(II) sulfate solution * Zinc Powder * 1 Thermometer * 1 Stopwatch * Weighing Boat * Electronic Balance VARIABLES:
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