Calorimetry and Specific Heat Tessa Williams Chemistry 111 11/13/13 Abstract: In this experiment‚ the specific heat and the density of an unknown metal was determined in order to identify the unknown metal. The average specific heat of the unknown metal was 0.197˚C and was determined using a calorimeter. The density of the unknown metal was 6.57 g/mL and was determined using a cylinder and displacement. Using the specific heat value of the unknown metal and its density‚ it
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Abstract The phenomenon of evaporative cooling is a common process in nature‚ whose applications for cooling air are being used since the ancient years. In fact‚ it meets this objective with a low energy consumption‚ being compared to the primary energy consumption of other alternatives for cooling‚ as it is simply based in the phenomenon of reducing the air temperature by evaporating water on it. This process can be an interesting alternative to conventional systems in these applications where
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features prevent insects from entering the bag. 4. CP of apple cider = 3.651 Amount of energy in 1 kg of 100°C water = 419.04 KJ Amount of energy in 1 kg of 100°C water = 2676.1 KJ Energy difference = 2676.1 KJ – 419.04 KJ = 2257.06 KJ Enthalpy to convert 1kg of 100°C water to dry steam = 2257.06 KJ
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such as temperature and pressure‚ occur. The coefficients for helium and carbon dioxide were determined using a Joule-Thomson apparatus that created constant enthalpy within the system. Using literature values for the coefficients at room temperature‚ the experimental results allow examination of each gas’s unique nature. Introduction Enthalpy is a critical study in thermodynamics. It is a measurement of a system’s internal energy (U) and work associated with pressure and volume: H = U + PV
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Chem Final Exam Combination Combination reactions‚ also known as synthesis reactions‚ involve the combination of two or more substances into a single new substance: A + B ---> AB Many metal oxides‚ for example‚ absorb carbon dioxide (CO2) from the air to form carbonates: CaO(s) + CO2(g) ---> CaCO3(s) Decomposition Decomposition reactions represent the reverse of the combination process in that one substance breaks down into two or more substances: AB ---> A + B Water‚ or H2O‚ for example
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the deicer lab was to successfully conduct experiments to determine the usefulness of magnesium chloride as a deicer. To find how successful magnesium chloride is as a deicer‚ experiments were conducted to determine the freezing point depression‚ enthalpy of dissolution‚ the impact on the surrounding environment‚ and also the expenses of using magnesium chloride as a deicer. For magnesium chloride to be determined as a good deicer‚ the reaction with water needs to be exothermic so ice’s freezing point
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Entropy Spontaneous Reactions: reactions that given the necessary Ea‚ proceed to completion without continuous assistance Enthalpy and Spontaneity * exothermic reactions tend to be spontaneous * Endothermic reactions can be either * Electrolysis of water is non-spontaneous it will stop if you stop the supply of energy * DD reaction between ammonium nitrate and barium hydroxide is spontaneous‚ even through the Entropy * Measure of disorder or randomness * Can apply to
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ST ANDREW’S JUNIOR COLLEGE JC 2 Preliminary Examination CHEMISTRY 9647/03 Higher 2 13 September 2010 Paper 3 Free Response 2 hours Candidates answer on separate paper. Additional Materials: Answer paper‚ Graph Paper‚ Data Booklet READ THESE INSTRUCTIONS FIRST Write your name and civics group on all the work you hand in. Write in dark blue or black pen on both sides of the paper. You may use a soft pencil for any diagrams‚ graphs or rough working. Do not use staples‚
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the space below. Also include any observations you made over the course of Part II. Calculations: Show your work and write a short explanation with each calculation. Part I: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. The water has absorbed the heat of the metal. So‚ qwater = qmetal Using the formula qmetal
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pressure. Isentropic Efficiency Due to irreversibility’s in a real turbine‚ the actual work transfer will be less than in an ideal machine and consequently the specific enthalpy at exit will be higher than the isentropic enthalpy. Isentropic Efficiency = Shaft power/Isentropic power The shaft power and the isentropic enthalpy change rate can be found from respectively‚ Ps = τ.ω = F.r.ω ∆H = m.Cp.∆T TPy-1/y = Constant Setup In a single stage radial reaction turbine the inlet gas is flown
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