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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Experiment 12 Calorimetry and Heat of Reactions ____________________________________________________________________________________________________________ PERFORMANCE GOALS: 1. To learn how to use of a calorimeter 2. To learn how to collect and manipulate data in the computer 3. To calculate the calorimeter constant 4. To use Hess’ Law to find the heat or formation of magnesium oxide CHEMICAL OVERVIEW: • Enthalphy: (ΔH) : when chemical or physical changes occur at a constant
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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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Module 3: Kinetics of Chemical Reactions Introduction to Kinetics Chemical thermodynamics has answered the question “can a specified chemical reaction take place?” (i.e. is the reaction thermodynamically favourable?). • However‚ chemical thermodynamics hasn‟t answered the question “HOW FAST will a specified chemical reaction occur?” o Many thermodynamically favourable reactions are so slow (ex: metamorphic transformation of rocks‚ corrosion of marble sculptures owing to weathering) that they can
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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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Abstract Density functional theory (DFT) calculations have been used to investigate the structural properties‚ dipole moments‚ polarizabilities‚ Gibbs energies‚ hardness‚ electronegativity‚ HOMO/LUMO energies‚ chemical potentials‚ density of states and detonation properties of trans and cis configurations of azocubane. All properties have been obtained using the B3LYP functional and 6-31G(d‚p) basis set. Also‚ IR‚ UV-Vis‚ CD and NMR spectra of the structures were simulated. The volumes of the structures
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dissolves in solution. A more a substance dissolves‚ the higher the Ksp value it has. In this experiment‚ a system of a sparingly soluble salt in water is studied. From the solubility information at various temperatures‚ the changes in standard enthalpy‚ standard entropy‚ and standard free energy were established. II. THEORETICAL BACKGROUND The reaction that is studied in this experiment is the dissolution of borax in water. “Borax” is a naturally occurring compound; it is in fact the most
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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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