R.L. DENUMIREA POSTULUI DE MUNCA: ORGANIZATOR DE SPECTACOLE COD COR: 342909 Obiectivele specifice ale activitatii de munca: - elaborarea proiectelor de spectacol; - negocierea cu furnizorii de servicii; - coordonarea activitatilor de pregatire si desfasurare ale spectacolului; - mentinerea permanenta a contactului cu coordonatorul departamentului. INTEGRAREA IN STRUCTURA ORGANIZATORICA Pozitia postului in cadrul structurii organizatorice: - Postul imediat superior: coordonatorul de organizare
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(or Mass) | Concentration (or Molar Mass) | Cu(NO3)2 (aq) | Light blue solution | 10 ml | 0.10 M | NaOH (aq) | Clear solution | 20 ml | 2 M | HCl (aq) | Clear solution | 20 drops | 6 M | NH3 (aq) | Clear solution | 7 drops | 6 M | H2SO4 (aq) | Clear solution | 15 ml | 1.5 M | Zn dust | Silvery substance | 0.15 g | | ethanol | Clear solution | 5 ml | | Volume of Cu (NO3)2 (aq): 10 ml Concentration of Cu (NO3)2 (aq): 0.10 M Convert ml to l: 10 /
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and Complex Ion Equilibria → Ag + + 2 NH Ag(NH3 ) +2 ← 3 [Ag ][NH ] = [Ag(NH ) ] 2 + Kd 3 + 3 2 → Cu 2+ + 4 NH Cu(NH 3 ) 24+ ← 3 [Cu ][NH ] = [Cu(NH ) ] 4 2+ Kd Complex Ion Equilibria 3 2+ 3 4 3 Complex Ion Equilibria • A metal ion coordinated to several neutral molecules or anions forms compounds called complex ions. • Familiar examples of complex ions include: • • Ag(NH3 )+2 Cu(NH3 )+4 Complex ion equilibrium constants are called dissociation constants. Example: Calculate the concentration
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imediata apropiere a orasului cu acelasi nume‚ la o altitudine de 475-600 m. Oraş aflat pe cursul superior al râului Târnava Mică‚ în Depresiunea Praid-Sovata‚ la poalele dinspre sud-vest ale Munţilor Gurghiu (Carpaţii Orientali)‚ altitudine 475-530 m‚ 60 km est de municipiul Târgu Mureş (reşedinţa Judeţului Mureş). Se învecinează la nord cu dealul Cireşelu de 912 m‚ la est cu dealul Stejaru de 649 m‚ la nord-est cu dealul Becheci sau Bicheş de 1080 m‚ iar la nord-est cu Masivul Gurghiu‚ vârful Saca
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n n n n n 0 Cu Transition metal – different oxidation states Cu0 elemental state Cu+1 Cu+2 most common Cu+3/ Cu+4 unusual oxidation - 2 electrons 2+ Cu reduction + 2 electrons 0 Cu Objectives n To observe a sequence of chemical reactions starting and finishing in elemental copper metal‚ and to practice quantitative laboratory techniques. Cu → Cu(NO3)2 → Cu(OH)2 → CuO → CuSO4 → Cu Cu(NO3)2 = copper nitrate Cu(OH)2 = copper hydroxide CuSO4
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generează un fascicul coerent de lumină. Fasciculele laser au mai multe proprietăți care le diferențiază de lumina incoerentă produsă de exemplu de Soare sau de becul cu incandescență: * monocromaticitate — un spectru în general foarte îngust de lungimi de undă; * direcționalitate — proprietatea de a se propaga pe distanțe mari cu o divergență foarte mică și‚ ca urmare‚ capacitatea de a fi focalizate pe o arie foarte mică; * intensitate — unii laseri sînt suficient de puternici pentru a fi
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reciprocal. If a reaction step is multiplied by a common coefficient n‚ the new equilibrium constant is raised to the nth. The first part of the experiment dealt with the equilibrium reaction Cu(OH)2(s) ⇌ Cu2+(aq) + 2OH-(aq). 0.10 M Cu(NO3)2 and 0.10 M NaOH were reacted together in seven test tubes to form the solid Cu(OH)2‚ a blue precipitate. Distilled water was added to the first test tube. This served as the control. When 6.0 M H2C2O4 was added to the second test tube‚ the precipitate turned cloudy
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(Caulk) – admixture of spherical Ag-Cu eutectic particles with conventional lathe-cut – eliminated gamma-2 phase Classification According to content – Silver amalgam: Silver more than 65% – Copper amalgam: 70% Hg and 30% Cu According to presence or absence of Zn Zinc containing alloys – more than 0.01% Zn Zinc free alloys – less than 0.01% Zn Classification • According to Copper content – Low copper alloys (2-4-6% Cu) – High copper alloys (9-30% Cu) According to the shape of alloy
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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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