Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy D. F. Nachman 6/23/2010 Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M sulfuric acid solution: Mg(s) + H2SO4(aq) →MgSO4(aq) + H2(g). We found the experimental molar enthalpy of reaction to be ΔH = –355 ± 17 kJ/mol at 0°C‚ 24% lower than the textbook value of ΔH° = –466.9 kJ/mol‚ reported at 25°C. Introduction Whether a chemical reaction occurs spontaneously or is driven by an outside
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of Kennecott using FCFcap is: $53.8 Value of Kennecott using FCFeq is: $49.91 Steps using FCFcap: Step 1: FCF_cap=EBIT(1-t)+depreciation+ amortization -Capex-change of NWC =NI+Interest(1-t) - Change of Net PPE - Change of NWC Step 2: WACC calculation: WACC=%Equity * Re + %Debt*Rd*(1-t) Re=Rf+beta*MRP=15.8% So‚ WACC= 65%*15.8%+35%*10%*(1-0.5)=12.03% Step 3: Multiply FCF with corresponding discount factors (1/(1+WACC)^n) PV(FCFcap)= 166.12 Step 4: Terminal value of equity = 116.2*10 – 117
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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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5-1 Earned Value Calculation 1. PV-BCWS=$3607.14 EV-BCWP=$3593.34 (.98 x 3666.67) CPI x AC AC-ACWP=$3666.67 (3593.34/.98) EV/CPI 2. SV= -13.8 (3593.34 – 3607.14) EV – PV CV=73.33 (3593.34 – 3666.67) EV – AC SPI=1.0 (3593.34/3607.14) EV/PV CPI=.98 (3593.34/3666.67) EV/AC 3. According to these calculations‚ the schedule variance is running late and the cost variance did not run over. The SPI is 1.0 which means that it is running on schedule. The CPI is .98 which is over budget by
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Experiment 1: Synthesis of Copper Compounds Introduction This experiment involves the synthesis of compounds originating from pure solid copper. By applying solubility rules and the reactive properties of substances‚ many compounds which would otherwise be costly to extract from nature are able to be synthesized in the laboratory. Laboratory synthesized may sometimes be more economical than natural extraction‚ however it poses its own problems with the amount of substance that is actually yielded
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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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Measuring the enthalpy change of vaporisation of water You should attempt this part of the activity even if you have not seen the demonstration of the practical. 1. Calculate a value for ∆Hvap for water in KJ mol-1 using the data from the demonstration. Also‚ calculate ∆Hvap from the following data gathered by a student; 8100 J were needed to distil 2.95g of water. a) Explain why the boiling tube was surrounded with expanded polystyrene (or other similar insulation)‚ but the condenser was left
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How to Calculate Preferred Dividends Preferred stock (or preference shares) is a special class of stock that pays a fixed dividend set at the time of issuance. Also‚ preferred dividends must be paid before common stock dividends. To calculate the dividends for preferred stocks‚ you need to multiply the par value of the shares by the dividend percentage. Example 1: If the dividend percentage is 8 percent and the preferred stock was issued at $20 per share‚ then the annual dividend is: 8% * $20 =
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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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KENNECOTT COPPER CORPORATION CASE REPORT 1. Analyze the economic rationale of the Carborundum acquisition. Under what conditions an acquisition would be expected to add to shareholder value in general? Do any of these reasons apply to Carborundum acquisition? Prior to the consideration of Carborundum as an acquisition target‚ Kennecott‚ a copper company‚ pursued an acquisition of Peabody‚ a coal company‚ for $285 million in cash in 1968. There are two main rationales behind the acquisition of
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