Determining the composition of pennies with redox reactions Introduction: The understanding of oxidation and reduction must be clear to carry out this lab. With the understanding of these concepts we can calculate or hypothesize for the properties of each element or compound. Oxidation involves the gain of electrons of hydrogen or the loss of oxygen or decrease in oxidation state. If zinc completely reacts with HCL‚ then the theoretical yield of copper should be equivalent to the actual yield
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half-equations given the species involved in a redox reaction. Example: Zn + Cu2+ → Zn2+ + Cu Oxidation: Zn → Zn2+ + 2e Reduction: Cu2+ + 2e → Cu 9.2.2 Deduce redox equations using half-equations. Example: NO3- + Cu → NO + Cu2+ 1. Balance atoms other than H and O Cu → Cu2+ NO3- → NO 2. Balance O by adding H2O as needed NO3- → NO +2H2O 3. Balance H by adding H+ as needed 4H+ + NO3- → NO +2H2O 4. Balance charges by adding e Cu → Cu2+ + 2e 3e + 4H+ + NO3- → NO + 2H2O 5. Equalise electrons in half equations
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ENGINEERING CHEMISTRY –II UNIT-I Electrochemistry Principles Redox reactions Redox stands for reduction-oxidation‚ and are electrochemical processes involving electron transfer to or from a molecule or ion changing its oxidation state. This reaction can occur through the application of an external voltage or through the release of chemical energy. Oxidation and reduction Oxidation and reduction describe the change of oxidation state that takes place in the atoms‚ ions
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Copper‚ Cu Lead‚ Pb Zinc‚ Zn Magnesium‚ Mg The following solutions: Copper (II) nitrate‚ Cu(NO3)2 Lead (II) nitrate‚ Pb(NO3)2 Zinc nitrate Zn(NO3)2 Magnesium nitrate‚ Mg(NO3)2 Silver nitrate‚ AgNO3 Fine sandpaper Goggles Lab apron Directions: Fill in your observations from the videos and pictures in the table below. DATA TABLE Aqueous Nitrates Metals Mg(NO3)2 Zn(NO3)2 Cu(NO3)2 Pb(NO3)2 AgNO3 Mg Zn Cu
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student reacted 2.8 grams of Fe (s) (steel wool) in excess CuSO4 (aq)‚ according to the following balanced equation: Fe(s) + CuSO4 (aq) -> FeSO4 + Cu(S). When the Fe(s) was completely consumed‚ the precipitated Cu had a mass of 3.2 grams. Did the student’s result on this experiment verify the mole ratio of Fe(s) to Cu as predicted by the equation? Answer: yes‚ because the experiment result was 2:1 Calculate the mole ratio of Fe to Cu and explain Ase
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Cu2+ (aq) + Zn (s) Cu (s) + Zn2+ (aq) E°cell = 1.06 V Cu2+ (aq) + 2e-
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before tests can be conducted.. CATion ammonium zinc Reaction with aqueous Sodium Hydroxide NO ppt. Ammonia gas produced on warming. White ppt. [y] Soluble in excess aq. NaOH to form a colorless solution. [z] Zn2+ + 2OH- Zn(OH)2 (white ppt) Zn(OH)2 + 2OH- [Zn(OH)4]2- (aq) White ppt. [u] Ca2+ + 2OH- Ca(OH)2 (white ppt) Insoluble in excess aq. NaOH. [w] White ppt. [p] Soluble in excess aq. NaOH to form a colorless solution. [q] Al3+ + 3OH- Al(OH)3 (white ppt) Al(OH)3 + OH- [Al(OH)4]-
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copper ions. this is the balanced equation for the reaction Cu(s) + 4H+(aq) + 2NO3-(aq)---> Cu2+(aq) +2NO2(g) + 2H2O(l) The reaction of aq copper nitrate with sodium hydroxide was the turning of the solution to a blue color‚ when water was added a cloudy mass of blue was formed below. This precipitate was copper (II) hydroxide. The precipitate was blue because of the copper ions. the balanced equation for this is Cu2+(s) + 2OH-(s) ---> Cu(OH)2O(s) The third reaction copper (II) hydroxide solution
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SOLUTION MINING A Laboratory Exercise in Extracting Copper from a Synthetic Copper Ore Your Name __Mel Hine______________________ Partner’s Name __Jay Ranson____________________ Date _October 2‚ 2012____________ Introduction This laboratory exercise involves the use of dilute sulfuric acid (H2SO4) to leach copper
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agricultural‚ commercial and industrial waste] as adsorbents for pollution abatement have been investigated extensively in recent years. The non conventional adsorbents process remarkable adsorption capacity for the removal of heavy metals like Cd‚ Cr‚ Cu‚ Fe‚ Hg‚ Mn‚ Ni and Pb‚ surfactants‚ dyes‚ colour‚ organics from the industrial and municipal effluent. This paper represents the review of past work on removal of heavy metals by biosorption by using low cost adsorbents in natural and modified forms
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