Examples of synthesis reactions: 1. Metal + oxygen → metal oxide EX. 2Mg(s) + O2(g) → 2MgO(s) 2. Nonmetal + oxygen → nonmetallic oxide EX. C(s) + O2(g) → CO2(g) 3. Metal oxide + water → metallic hydroxide EX. MgO(s) + H2O(l) → Mg(OH)2(s) 4. Nonmetallic oxide + water → acid EX. CO2(g) + H2O(l) → ; H2CO3(aq) 5. Metal + nonmetal → salt EX. 2 Na(s) + Cl2(g) → 2NaCl(s) 6. A few nonmetals combine with each other. EX. 2P(s) + 3Cl2(g) →
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observe how the change in solvent polarity affects the rate and to determine the kinetics of a solvolysis reaction. In this experiment‚ we used 1-chloro-1-phenylethane in acetone in one reaction with 50% ethanol-50% water and in another reaction with 40% ethanol-60% water. To monitor he rate of reaction‚ we would need the concentration of the alkyl chloride at the beginning of the reaction and at a time t‚ but since we did not determine the concentrations‚ we monitored the rate of formation of
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Introduction The purpose of this experiment is to determine the rate equation for the “Iodine Clock Reaction” experiment. The experiment will consider the equations 〖2I〗^-+S_2 O_8→2〖〖SO〗_4〗^(2-)+I_2 and I_2+2〖S_2 O_3〗^(2-)→2I^-+S_4 O_6 in order to determine the rate law of Rate=k[〖〖S_2 O_8〗^(2-)]〗^a 〖[I^-]〗^b by using the experimental data to calculate the values of exponents a and b as well as the rate constant k. Experimental Supplies Needed: 250 mL Erlenmeyer flask‚ 100 mL beaker‚ graduated
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laboratory assignment 3 was to measure the rate at which a chemical reaction takes place. For the purpose of this lab we measured the rate a balanced oxidation/reduction reaction between iodine‚ hydrogen‚ and bromate ion occurs. The above reaction occurs slowly so we used a coupled iodine clock reaction to measure the rate of the oxidation/reduction reaction because it occurs much faster but is still dependent upon the other reaction. To accomplish this‚ two mixtures were prepared in separate Erlenmeyer
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Measuring Human Reaction Time Name: Prerna Mohan Date: November 3‚ 2017 Team members: Allison Fitzgerald‚ Isabella Federico 1. Objectives The objective of this lab is to measure each individual’s reaction time using a ruler. 2. Method and Equation: We will apply free fall kinematics to find our own reaction time. An object in free fall is an object in motion where gravity is the sole force acting upon it. If we drop an object from a certain distance‚ the object will experience constant
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tubes. In another set of test tubes‚ 0.1 and 0.2 ml of the extract were taken. In each test tube‚ the volume was made up to 1 ml‚ followed by addition of the prepared alkaline solution (5 ml) at room temperature. The solutions were left undisturbed for 10 minutes. Then‚ 0.5 ml of Folin-Ciocaltcau reagent was added rapidly. They were incubated at room temperature for 30 minutes until a blue colour appeared. Before taking the readings of the standard and the samples‚ the spectronic
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the limiting reactant of a chemical reaction that involves iron filings and a copper sulfate solution. Second‚ to determine the mole ratios between iron and copper and to show that a single replacement reaction occurs when iron and copper sulfate react with each other. And lastly‚ to determine/calculate the percent yield to better analyze the chemical reaction between iron and copper sulfate to produce copper and iron sulfate. The method used to perform this lab will be to combine a metal with a solution
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Concentration vs Rate of reaction Brandon Introduction A reaction rate is the speed at which a chemical reaction will occur. Heat‚ concentration of a chemical‚ Surface area or a catalyst‚ will affect the rate of reaction. The concentration of a chemical will speed up of the reaction because the reactant particles have become more crowded therefore increasing the chance of productive collisions. In this practical the chemicals will be Sodium thiosulphate and Hydrochloric acid which will produce
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|Zn |Mg |Cu |Pb | | |(+) clear liquid but the |(+) a black spot appeared on|(-) no reaction occurred |(-) no reaction | |Pb(NO3)2 |Zinc itself turned glittery |the sliver of magnesium. | | | | |(+) the liquid looks |(+)
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purpose of this lab was to find the theoretical and experimental percentage yields of the double displacement reaction between the solutions Lead (II) Nitrate (PbNO3) and Potassium Iodide (KI). It is important to obtain amounts of Lead (II) Nitrate and Potassium Iodide as close to 1.44g as possible. This reaction creates Lead (II) Iodide and Potassium Nitrate. The precipitate during this reaction is Lead (II) Iodide. The balanced equation is Pb(NO3)2 + 2KI= PbI2 + 2KNO3. In this lab the Lead (II) Iodide
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