I found out how to get the formula of Mg + 1/2 O2 ---> MgO... The only thing is that I didn’t find the (delta) H for the target formula. I believe you can find it using the appendix of your book ( assuming they want you to find the Standard Enthalpies of Formation for the other formulas ).... For my rference to them in this answer‚ I substituted the values with variables.... To find Mg + 1/2 O2 --> MgO‚ (1) Mg + 2HCl --> H2 + MgCl2 (delta) H = X (2) MgO + 2HCl --> H2O + MgCl2 (delta) H
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Vapor Pressure and Enthalpy of Vaporization of Water 1/9/12 Emily Toy Lab Partner: Zack Ronnei Instructor: Ms. Olsen‚ AP Chemistry Purpose: The purpose of this lab is to find the vapor pressure of water at temperatures between 50oC and 80oC. Procedure: 1. Take a10 mL graduated cylinder and fill it with 7 mL of water. 2. Next fill a 1000 mL beaker ¾ full with water. 3. Cover the graduated cylinder by putting your finger on top and place the cylinder in the 1000 mL beaker. Make
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xam 2 [pic] Summer 2011 Chemistry 1411 EXAM # 2 Activity Series of Metals in Aqueous Solution [pic] CHEM 1411 Exam # 2A Name:________________________________ (Chapters 4‚5‚6‚ and 7) Score: [pic] Part I- ( 3 points each) - Please write your correct answer next to each question number‚ DO NOT CIRCLE. ____ 1. Compare the rates of effusion of CO2 & SO2‚ rCO2/rSO2 A. CO2 will effuse 1.45 times
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Combustion of Alcohols Purpose: The purpose of this investigation is to use calorimetry to determine the molar enthalpy change in the combustion of each of a series of alcohols. Question: How do the enthalpies of combustion change as the alcohol molecules become larger? Prediction: I predict the bigger the molecule the more the energy will be released. Materials: On lab sheet Procedure: On lab sheet Observation: On other page Analysis: b) i) Ethanol – q=(100g)(4.18J/g/C)(25.5C) q=10659J
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p IB DIPLOMA PROGRAMME PROGRAMME DU DIPLÔME DU BI PROGRAMA DEL DIPLOMA DEL BI Chemistry Higher level and standard level Specimen paper 1s‚ 2s and 3s For first examinations in 2009 CONTENTS Chemistry higher level paper 1 specimen paper Chemistry higher level paper 1 specimen markscheme Chemistry higher level paper 2 specimen paper Chemistry higher level paper 2 specimen markscheme Chemistry higher level paper 3 specimen paper Chemistry higher level paper 3 specimen markscheme
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Determination of the Enthalpy for Decomposition of Hydrogen Peroxide Objective: To construct a coffee cup calorimeter‚ measure its calorimeter constant‚ and determine the enthalpy of decomposition and formation of hydrogen peroxide. Background: This experiment is a classic thermodynamics lab. In it‚ we attempt to measure the enthalpy (H) of a chemical reaction. The main obstacle is that this is a quantity that cannot be measured directly. It instead is observed as heat from one substance is transferred
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chemical reaction occurs in which the system produces heat it is exothermic (it feels hot) Under conditions of constant pressure the heat absorbed or released is termed enthalpy (or "heat content"). We do not measure enthalpy directly‚ rather we are concerned about the heat added or lost by the system‚ which is the change in enthalpy (or ΔH The quantity of heat gained or lost by a system‚ ΔH‚ is dependent upon‚ the mass‚ m‚ of the system: the more massive an object the more heat needed to raise its
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Determining an enthalpy change of a displacement reaction Aim: To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution. Zn (s) + Cu2+ (aq) → Cu2+ (s) + Zn2+ (aq) Theory: For the displacement reaction‚ an excess amount of zinc powder is added to the measured amount of aqueous copper (II) sulphate. The temperature change over a period of time has to be measured and thus‚ the enthalpy change for the reaction can be measured. The equation
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Chemistry Internal 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
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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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