Exercice 2-5->(a) Calculer le AG° à 25°C relatif à la réaction CH3CH2Cl → CH2=CH2 + HCI (c'est la réactionde l'exercice 2.2 considérée à l'envers). (b) Pour la même réaction, calculer le AG° à 500°C.TAS sans oublier de convertir préalablement les degrés(Indication: appliquer AG = AH°Celcius en kelvins.)

Step 1:To calculate the Gibbs free energy change (ΔG) for the reaction CH3CH2Cl⇌CH2=CH2+HCl at…

Answered: Exercice 2-5 -> (a) Calculer le AG° à…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 9RQ: What characterizes an electrolytic cell? What is an ampere? When the current applied to an...

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What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Can you show me how to solve this or
Indicate whether the following reactions will occur spontaneously or not. (a) Ni²*caq) + Pb)→ Nio) + Pb²*(a) (b) 3FE²*(mq) + 2Cre)→ 3Fe«)+ 2Cr³*(»q) (c) 2Agʻ(»q) + Crs)→ 2Ags) + Cr²"(aq)
105
DG° < 0, DH° < 0 and DS° < 0 is it this if the reaction is H2O (l) →→ H2O (s) occurring at -20°C and standard conditions..
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10-4-1. answer on bracket thanks
4.) For the following equilibrium reaction state what happens when the following reagents are added NaOH(aq) + HСІ(ад) + НОН(аq) + NaCI(aq)+д a.) Mg(ОН)2 b.) КCІ с.) KBr d.) Heat (A) e.) CH;CH,COH (an acid) f.) decrease in temp.
Calculate AH° for the reaction 2K (s) + 2H,0(1) — 2КОН(аq) + Hә (9) Substance and State AHF° (kJ/mol) K(s) KOH(ag) H2 (g) H2O(1) -481 -286 ΔΗ' kJ
Calculate the equilibrium constant (Kc) for the following reaction: CH3COOH(aq) + OH-(aq)) CH3COO-(aq) + H2O(l) The Ka of acetic acid is 1.75 x 10-5; Kw for auto-ionization of water = 1 x 10-14 Hint: First write the equilibrium expressions for both species (reactants) separately then apply manipulation rules of K and find the answer)
Determine the AH of the reaction 1 1 NO29) + 702c9) +5H20(9) → HNO3(aq) 4 AH = 33.2 kJ 5 N2c9) + O2cg) → N02c9) 1 Haa) +Nzo) +0zc) → HNO3(aq) AH = -202.3 kJ 1 H2(g) - ΗΝO3(αq) 1 H2(g) * 2 → H20(g) AH = -285.8 kJ

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