14 may be a possible EEC. Moreover‚ the calculated compensation temperature by inverting the straight line slope‚ T comp = 57.9 ºC‚ is higher than the average experimental value‚ T exp = 32.5 ºC. This great difference between these two values of temperatures might reflect the existence of real EEC rather than experimental error [58]. Another evidence of EEC is the approximate constant ∆G # with a significant change in both ∆H # and ∆S # . Finally‚ EEC was also investigated by using
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with copper‚ Cu‚ the oxidation number of silver (Ag) ions that form will be +1. The unbalanced chemical equation that we used to represent this reaction is Cu + AgNO3 → Ag + Cu(NO3)2. In order to find the approximate masses of reactants needed to produce about 2 grams of silver‚ we found the molar masses of each of the reactants and products: Molar Masses | |AgNO3 |Cu |Ag |Cu(NO3)2
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tehnicilor de înregistrare cu dispozitive de tipul MEA (Micro Electrode Area). Aceste cercetări au permis progrese şi în domeniile maladiilor precum cancerul şi Parkinson. Înregistrările făcute cu MEA‚ permit descifrarea (parţială) a mecanismelor şi modului de funcţionare a diverselor zone corticale. La ora actuală au fost dezvoltate mai multe tehnologii de tip fotolitografic pentru imprimarea ariilor de microelectrozi fie pe suporturi solide (de
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zinc and copper mixtures‚ which have 11 groups. Determining the volume of the zinc and copper mixtures each‚ and record the data. Using equation get the density of the pennies. Compare the results. Find the best-fit straight line. Material: 0%Cu—100%Cu 0%Zn—100% Zn 5‚ 10‚ 20‚ and 30 pre 1982 pennies. 5‚ 10‚ 20‚ and 30 post 1982 pennies. Graduated Cylinder Procedure: Weight the mass of the different percentages of zinc and copper mixtures. Determining the volume of the different percentages
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experimental method produces more accurate result. One was electrochemistry using a Daniel cell and the other one was spectrometry by estimating concentration of complex solution using a calibration curve. The formation constant of cupric ammine complex Cu(NH3)42+‚ Kf‚ came out with 1.93x10^15 using electrochemical cell method and 9.79x10^12 using spectrophotometer method. Considering the literature value of Kf is around 4.8x10^12 ~ 1.7x10^13‚ spectrophotometer gives more accurate result than electrochemical
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solution. Most solids that are commonly referred to as "insoluble" are actually slightly soluble and will produce an equilibrium between undissolved solid and ions in solution. For example‚ when copper (II) iodate (Cu(IO3)2) is placed in water‚ the following equilibrium is established. ( 1 ) Cu(IO3)2(s) Cu2+(aq) + 2 IO3-(aq) The equilibrium constant associated with this reaction is called the solubility product constant and is given the symbol Ksp. ( 2 ) Ksp = [Cu2+][IO3− ]2 It is important to
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colorimetry. Anhydrous copper sulfate (CuSO4) is white‚ which means that it does not absorb light in the visible region of the spectrum. The hydrated copper sulfate (CuSO4 - 5H2O) is blue. The structure of the compound can be represented more accurately as Cu(H2O)4 SO4 - H2O where four water molecules are bound to the copper ion and the fifth is a water of crystallization. The water molecules are arranged at the corners of a square‚ with the copper at the center. Such an arrangement is called square coplanar
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avoc ado & cu cu mber/ t o biko. 8 SEARED HAMACHI aged m is o‚ mic ro was a b i ‚ p i c k l e d j a l a p e no. 9 ALASKA sal mon‚ avoc ado & cu cu mber. 8 NEW YORK shr imp‚ avo c ado & cu cu mber. 8 SALMON SKIN sal mon skin‚ cu cu mber‚ shiso‚ kaiw are‚ gob o & ponz u. 8 ROCK ‘N ROLL bbq eel ‚ avo c ado & cu cu mber/ eel sauc e. 8 SPICY TUNA‚ HAMACHI‚ OR SCALLOP cu cu m b e r & ka iwa re. 9 TEMPURA SHRIMP kaiw are & avo c ado / sp ic y aio l i. 11 DRAGON t emp u r a shr imp‚ cu cu mber & avo
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evolution or absorption of heat or even change in color. This experiment aims to observe the different chemical changes copper undergoes in different conditions. II. METHODOLOGY 1. Precipitation of Copper (II) Hydroxide Materials used: 0.100 M Cu(NO3)2 solution‚ 250-mL beaker‚ 6.00
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appearance of metallic deposits on the surface of the metal stip. TABLE 1: Chemical Reaction SOLUTION and METAL EVIDENCE of REACTION PRODUCT 1. AgNO3 + Cu deposits of Ag —> Ag + Cu(NO3)2 2. Cu(NO3)2 + Pb deposits of Cu —> Cu + Pb(NO3)2 3. Pb(NO3)2 + Zn deposits of Pb —> Pb + ZnNO3 4. MgSO4 + Zn no reaction —> no reaction 5. HCl2SO4 + Cu no reaction —> no reaction 6. HCl2SO4 + Zn deposits of H —> H2 + ZnCl2 TABLE 2:
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