Ziadat | | | Title: Investigating the effects of changing the concentration of an acid on the rate of reaction between HCl and Magnesium. Aim: In this experiment we are going to see the effects of using three different concentrations of HCl when added to Magnesium metal on the rate of reaction. Hypothesis: If the concentration of the acid increased in reaction between HCl (the acid) and magnesium‚ then the rate of reaction will increase. Scientific background: For many reactions involving liquids
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Observations Part I: Equilibrium Involving Thymol Blue Table 1 Reagent Added | Stress (Ion Added) | Colour Observation | Direction of Equilibrium Shift | NaOH (Step 5) | OH⁻ | Green | Left | NaOH (Step 6) | OH⁻ | Blue | Left | HCl (Step 3) | H⁺ | Green | Right | HCl (Step 4) | H⁺ | Yellow | Right | Part II: Equilibrium Involving Thiocyanatoiron (III) Ion Table 2 Reagent Added | Stress (Ion Added) | Spectator Ion | Observation | Direction of Equilibrium Shift | KCl | None | K⁺‚ Cl⁻ |
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instructor. III. Pre-lab Questions 1. Define ΔHrxn. ΔHrxn is enthalpy of products – reactants. (ΔHrxn = Hprod-Hreact). 2. In today’s lab you will be using 50.0 mL of 2.0 M HCl. Using Equation 3 (M=mol/L) from above‚ calculate the number of moles of acid used. M=mol/L 2.0M = x / 0.0500L x = 0.10 mol HCl 3. You will also be using 50.0 mL of 2.0 M NaOH. How many moles of base are used? M=mol/L 2.0M = x / 0.0500L x = 0.10 mol NaOH 4. The specific heat of a solution is 4.18 J/g
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To learn how to measure the volume of a liquid using a buret. Prelab Questions: 1. Calculate the number of moles in 2.65g of zinc. 2. Calculate the number of moles of hydrochloric acid in 37.5mL of a 3.00M HCl solution. 3. Calculate how many moles of HCl are required to react with 0.244 moles of zinc. Procedure: 1. Put on safety equipment. 2. Label small glass vial so your group can identify it later. 3. Determine the mass of the clean dry vial and record
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reaction 2 HCl(g) +I2(s) [pic] 2 HI (g) + Cl2(g) has Kc = 1.0 x 10-34 at 25˚C. If a 1.00 L reaction vessel initially contains 0.100 mol of each HCl and solid I2‚ what are the concentrations of HI and Cl2 at equilibrium? 2. Consider the following gas-phase reaction and equilibrium constant at 25 oC: 4 HCl(g) + O2(g) [pic] 2 Cl2(g) + 2 H2O(g) The concentrations of all species were measured at a particular moment in time and the following data were obtained: [HCl] = 0.00050
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Introduction: The students were handed 10 test tubes with no identification. The students were supposed to design a method in determining what chemical was in each test tube. The list of chemicals is CuSO4‚ NH4Cl‚ NaOH‚ AgNO3‚ KI‚ H2SO4‚ NaBr‚ CaCl2‚ HCl‚ and Pb(NO3)2. The students are expected to determine the chemicals using physical properties‚ litmus paper‚ solubility‚ and the process of elimination. Physical properties‚ such as the color‚ can be determined by sight. Litmus paper can be determined
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Joseph Corey‚ Chris‚ Grant Thermodynamics – Enthalpy of Reaction and Hess’s Law I. Purpose The purpose of this lab is to verify Hess’s Law through the three reactions of NaOH and HCl‚ NH4Cl and NaOH‚ and NH3 and HCl. The sum of the enthalpies of the first two reactions should equal the enthalpy of the third reaction. II. Background Hess’s Law is used to determine the enthalpy of a reaction from adding two or more preceding reactions. To determine the enthalpies of certain
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electrolyte‚ HCL‚ NaOH‚ NH4CL‚ NaC‚ conc.H2SO4; it contains a highconcentration of ions and so the bulb glows brightly. Introduction Substances that dissolve in water are either nonelectrolytes or electrolytes. Non-electrolytes are substances that do not form ions and are electrically non-conducting in solution. A common example is table sugar (sucrose) which dissolves in water as shown in Equation 1. Electrolytes are substances‚ such as NaCl and HCl‚ which form
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metals included in the lab. Materials: Apparatus Test-tube rack 4 test tubes (25 mm x 150 mm) 4 beakers (150 mL) Safety goggles Lab apron Plastic gloves Full face shield Reagents Zinc Magnesium Iron Copper 1M hydrochloric acid‚ HCl 1M sulphuric acid‚ H2SO4 1M acetic acid‚ HC2H3O2 1M phosphoric acid‚ H3PO4 Procedure: Please refer to Health Chemistry‚ Laboratory Experiments‚ page(s) 75-76. Data and Observations: Table 1: Comparison of Metal Activities Zinc
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reaction is endothermic. Materials 3 test tubes Test tube rack Solid cobalt chloride Distilled water Concentrated HCl Ice bath Hot water bath 10 ml graduated cylinder (for concentrated HCl) 2 droppers Spatula Tongs Digital balance Procedure 1.Label the test tubes 1-3. 2.Add 0.5g solid cobalt chloride to each test tube. 3.To test tube 1‚ add 4ml concentrated HCl. Use the graduated cylinder to transfer the acid. This will be your first control sample. What is the color of your sample
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