Determination of Reaction Enthalpy Shannon Wedepohl 9/17/13 Abstract: During this experiment‚ an ice calorimeter was used to measure the change in volume in milliliters of magnesium metal and 1.00 M of sulfuric acid. We found the experimental molar enthalpy of the reaction to be ∆H = -370 ± 1 kJ/mol at 0˚C. This compares with an expected value of -466.9 kJ/mol at 25 ˚C‚ a 20.75% difference. Introduction: Many chemical reactions truly only encompass changes by exchanging heat
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The 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)
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Step 1: Pb (NO3) 2 (aq) + CaCl2 (aq) PbCl2 (aq) + Ca (NO3) 2 (aq) (double displacement reaction) According to the solubility guidelines lead (II) chloride (PbCl2) is a possible precipitate. This is because even though most chlorides are soluble‚ lead chloride is considered insoluble (p.2‚ Lesson 17). Step 2: PbCl2 ↔ Pb2+ + 2Cl- Q = [Pb2+] [Cl-] 2 Step 3: Ksp = 1.2 x 10-5 (from table 17.1‚ p.5) Step 4: V2 = 20.0 mL (volume of Pb (NO3)2) + 45.0 mL (volume of CaCl2) = 65.0
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Assessment: Determining the Enthalpy Change of a Displacement Reaction AIM: To determine the enthalpy change for the reaction between copper(II) sulfate and zinc. BACKGROUND THEORY: Bond breaking is endothermic while bond forming is exothermic. The reaction between copper(ll) sulfate and zinc is exothermic as the energy required to form the bonds of the products is greater than the energy required to break the bonds of the reactants. In an exothermic reaction‚ heat is given off to the surroundings;
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air. The processes used to determine the molar concentration of sodium hydroxide was by: 1) using the volume of NaOH at the end point and 2) by using the volume of NaOH at the equivalence point. The pH meter was used for the end point and the second derivative and titration curve allowed us to get the volume of the equivalence point. The key difference between the end point and the equivalence point is that the end point is just an indicator of when the color changes and titration stops. The equivalence
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the Enthalpy of a Chemical Reaction All chemical reactions involve an exchange of heat energy; therefore‚ it is tempting to plan to follow a reaction by measuring the enthalpy change (∆H). However‚ it is often not possible to directly measure the heat energy change of the reactants and products (the system). We can measure the heat change that occurs in the surroundings by monitoring temperature changes. If we conduct a reaction between two substances in aqueous solution‚ then the enthalpy of
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calculate the enthalpy change of neutralization of the given pairs of acid and base. Theory: When alkali neutralizes an acid‚ a salt and water are formed. Aqueous hydrogen ions‚ H+(aq) from the acid react with the hydroxide ions‚ OH-(aq) from the alkali‚ forming water. Ionic equation: H+ (aq)+OH- (aq) → H2O (l) The identity of the salt will depend on the nature of the acid and alkali used. The combination of H+ and OH- ions in this way releases energy. In this practical‚ the enthalpy changes accompanying
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Title : Expt.1 Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Experiment no : 1 Experiment title : Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Objectives: 1) To understand the enthalpy chemistry. 2) To determine the calorimeter constant. 3) To determine the enthalpy reaction of acid-base reactions. 4) To study the exothermic reaction. Apparatus and Materials : * Dewar flask
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Calorimeter Determination of Reaction Enthalpy 9/11/2014 Introduction: A chemical reaction often indicated by a transfer of energy measured in heat. By measuring this heat transfer in a constant pressurized environment‚ the enthalpy of the reaction can be used to infer certain information about a specific reactions reactants and products. The transfer of heat from outside sources in would be described as an endothermic reaction. Contrary‚ when a reaction releases heat out to its surroundings
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Enthalpy of Neutralization Introduction Energy changes always accompany chemical reactions. If energy‚ in the form of heat‚ is liberated the reaction is exothermic and if energy is absorbed the reaction is endothermic. Thermochemistry is concerned with the measurement of the amount of heat evolved or absorbed. The heat (or enthalpy) of neutralization (∆H) is the heat evolved when an acid and a base react to form a salt plus water. Eq. 1 HNO2(aq) + NAOH(aq) → NaNO2(aq) + H2O(l) + Q Q in the
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