Effect of Particle Size solid zinc‚ approx. 0.5 cm × 2 cm‚ or solid marble chips zinc powder or calcium carbonate powder balance 2 test tubes 1M HCl (approx 10 mL per group) Part 2. Effect of Temperature 3 Alka Seltzer tablets 3 250-mL beakers water at three temperatures – with ice‚ room temperature‚ warm (around 70°C) Part 3. Effect of Concentration 1M HCl‚ 5 mL per group 3M HCl‚ 5 mL per group 6M HCl‚ 5 mL per group 3 pieces of zinc metal‚ each approx 1 cm × 1 cm 3 test
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the Cu-Zn voltaic cell used in the experiment. Zinc has higher reactivity and it is more likely to loss electrons. Thus‚ electrons flow from Zn electrode to Cu electrode. Copper stripe is the positive electrode. Zinc stripe is the negative electrode. Reaction happened on each terminal: Positive terminal: Zn-2e-→Zn2+ Negative terminal: 2H+2e-→H2 It is assumed that bubbles (hydrogen gas) will come out from copper electrode. It is assumed that zinc and copper stripes are pure. Classification of
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Reaction Criteria Assessed: Background Design Research Question What is the enthalpy change between the reaction of Zinc reducing Copper II ions? Purpose Determine the change in enthalpy for the redox reduction of zinc reducing Copper II ions. Independent Variable Dependent Variable The change in temperature Controlled Variables Materials/ Apparatus * Zinc powder * 2‚ Foam cups * 10 cm3 pipette * stopwatch * 1.00 M Copper II Sulfate * Scale * Scoop *
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Before the 1900s‚ tin was commonly used to package household foods. Since it protected the foods inside‚ and it could be bent with ease‚ it was regarded as an inexpensive‚ easy and health conscious way to keep foods fresh. Some of its disadvantages‚ which lead to its defeat to aluminum‚ included the fact that it could only be rolled thicker than aluminum; it became brittle when warm‚ reducing its malleability greatly‚ and the tin foil created a strange aftertaste‚ which was undesirable to many.
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the Repair of Deteriorated Concrete resulting from Reinforcing Steel Corrosion D. ASTM A615/A615M-09 Standard Specification for Deformed and Plain Billet-Steel Bar for Concrete Reinforcement E. ASTM B6-09 - Standard Specification for Zinc F. ASTM A82-07 Specification for Plain Steel Wire for Concrete Reinforcement PART 2 PRODUCTS 2.01 Materials PART 3 INSTALLATION PROCEDURE 3.01 Concrete Removal A. Undercut 10x10cm at the required location with the minimum
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Title “ The Effect of Various Metal Activity (Zinc (Zn)‚ Magnesium (Mg)‚ and Copper (Cu)) in the Color of Rainwater and Amount of Rust in the Iron Nail “ Hypothesis If the type of metal that has the highest activity will be used ‚ then there will be the least amount of rust found in the nail and the color of the rainwater would be the lightest. Independent Variable • Types of metals used in wrapping Title: “ The Effect of Various Metal Activity (Zinc (Zn)‚ Magnesium (Mg)‚ and Copper (Cu)) in the
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To find the redox reactions between a metal and dilute acid‚ metal-metal ion displacement and halogen displacement reaction. Materials: Test tubes (8)‚ pea size samples of the following metals; copper‚ lead‚ magnesium and zinc (10 ml)‚ 2M hydrochloric
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transportation equipment; roofing; chemical and pharmaceutical machinery; and alloys (brass‚ bronze and beryllium alloyed with copper are particularly vibration resistant); alloy castings; electroplated protective coatings and undercoats for nickel‚ chromium‚ zinc‚ etc. More recently copper is being used in medical equipment due to its anti-microbial properties. The United States has mines in Arizona‚ Utah‚ New Mexico‚ Nevada and Montana. Leading producers are Chile‚ Peru‚ China‚ United States and Australia
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other oxidation. A typical galvanic cell is based on the spontaneous redox reaction: Net Ionic Equation Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Half Equations Zn(s) → Zn2+(aq) + 2e– Cu2+(aq) + 2e– → Cu(s) The anode will undergo reduction (Zinc) and the cathode will undergo oxidation (Copper) The two half cells must be physically separated so that the solutions do not mix together. A salt bridge is used to separate the two solutions yet keep the respective charges in the solution from separating
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reaction occurred |(-) no reaction | |Pb(NO3)2 |Zinc itself turned glittery |the sliver of magnesium. | | | | |(+) the liquid looks |(+) There was also a black |(+) The copper almost looks |(+) the balls of lead turned| |AgNO3 |ash-like and the Zinc turned|spot that appeared on the |like fuzz grew on it |black and look fuzzy and
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