4. Un quimico mezcló soluciones de nitrato de hierro (III) y tiocianato de potasio para llevar a cabo la siguiente reacción:BerFe* (ac) + SCN- (ac)= FESCN*2 (ac)Si se encontró que las concentraciones molares en equilibrio de Fe*, SCN' y FESCN*2 son 5.32 x 10-4 M, 732 x 10 My6.78 x 10 M, respectivamente, ¿cuál es el valor de la constante de equilibrio?mo 1moles solutoM.moles= MxV(L)rapidez = k [A]*[B]"%3DV (L)solución[C[D][A] [B]TA]pH = pka + log[HA]y = mx + bpKa- log (Ka)Ka- 10-PkaE celda= EcitodoEanodo[0.0592 Vlog Q[CID[A]°[B]*E - EceldaO a. 178ОБ 174Oc. 187O d. 202

To calculate equilibrium constant we would use the given Concentrations of all Species at…

Un quimico mezcló soluciones de nitrato de hierro (II) y tiocianato de potasio para llevar a cabo la siguiente reacción: Fe (ac) + SCN (ac)= FESCN* (ac) Si se encontró que las concentraciones molares en equilibrio de Fe*, sCN' y FESCN? son 5.32 x 10 M, 732 x 10 My 6.78 x 10 M, respectivamente, zcuál es el valor de la constante de equilibrio? moles soluto M - moles - Mx V(L) rapidez = k [A}"[8p V (L)solución [CID] y= mx +b pH - pka + lo9 THA) pK - log (K.) K. - 10-Pka Erelda -Ecatodo-Einodo E - E'colda 10.0592 V log Q [CID O a 178 Оь 174 Oc 187 Od. 202

Un quimico mezcló soluciones de nitrato de hierro (II) y tiocianato de potasio para llevar a cabo la siguiente reacción: Fe (ac) + SCN (ac)= FESCN* (ac) Si se encontró que las concentraciones molares en equilibrio de Fe*, sCN' y FESCN? son 5.32 x 10 M, 732 x 10 My 6.78 x 10 M, respectivamente, zcuál es el valor de la constante de equilibrio? moles soluto M - moles - Mx V(L) rapidez = k [A}"[8p V (L)solución [CID] y= mx +b pH - pka + lo9 THA) pK - log (K.) K. - 10-Pka Erelda -Ecatodo-Einodo E - E'colda 10.0592 V log Q [CID O a 178 Оь 174 Oc 187 Od. 202

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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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.
What is a nonspontaneous reaction?
Use the values of AH to calulate AH for the follonng reactions. Substance and State AH (LJ/mol) Cag(PO,),(s) C&SO (s) CH,(G) HCN(9) HC(G) H,0(g) NH(9) NH,CI(s) 0,(0) HPO,(1) H,80,(1) 4126 -433 -75 135.1 -92 -242 -46 -314 -1267 -814 (2) + N OH 0O AH" b. Caa (PO), (s) + 31, SO.(1) + 3Ca$O.(s) + 2H,PO, (1) c NH3 (g) + HCIG) NH, CI(s) AH"= kJ 888
Which of the following reactions would have the most positive AS° value? A) SO,(g) + Na¸O(s) Na SO,(s) B) CO,(s) → CO,(g) C) Fe®*(aq) + SCN(aq) FESCN²"(aq) D) N,(g) + 3 H,(g) 2 NH,(g) E) 2 NO(g) + CI,(g) 2 NOCI(g)
Given the data in the table below, AHrxn for the reaction Ca(OH); + 2H;AsO4 → Ca(H;AsO4)2 + 2H;O is _ kJ. [A] -4219 (B] -130.4 [C] -4519 [D] -76.4 AH, (kJ/mol) -986.6|| Substance Ca(ОН), HASO, Ca(H;AsOa)2 -900.4 -2346.0 H;0 -285.9 O A В C D
(3) For the following reactions at 500 K: (a) PbS(s) + 02(g) Pb(s) + S02(8) (b) PbS(s) + 2P6O(s) → 3Pb(s) + SO2(g) calculate: (i) AH00, (ii) AS0, (iii) AG500, given the following information: PbS(s) 0,(8) Pb(s) SO, (g) PbO(s) -296 -219 Afjo. (kJ mol-) -94 AS0. (J K- mol-) 205 65 249 68 91 s00 In each case discuss briefly the feasibility of the reaction under the stated conditions and how the feasibility is influenced by temperature change. Calculate the reversal temperature where relevant assuming that Al and AS remain constant over the temperature range considered.
73. Given the following data Ca(s) + 2C(graphite) Ca(s) + ¿O,(g) CaO(s) + H,O(1) C,H,(2) + 0,(g) Clgraphite) + O,(g) CaC,(s) ΔΗ--62.8 k → CaO(s) AH = -635.5 kJ Ca(OH), (aq) AH = -653.1 kJ 2CO,(g) + H,O(1) AH = -1300. kJ CO,(g) AH = -393.5 kJ calculate AH the reaction CaC,(s) + 2H,O(1) → Ca(OH),(aq) + C,H¿(g) IS ONIA
Consider The Following Reaction: CaCO3(S) + 2HCl(Aq) = CaCl2(Aq) + H2O(L) + CO2(G) Write down the quation of the equilibrium constant kc for this reaction
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
Al(OH),(s) = Al³*(aq) +30H¯(aq) X x.- +. log, Cos, K = [AF][OH]; ОН
Calculate the K, of the reaction of Ag" binding with Ligand L Ag"(aq) + Llaq) → AgL*(aq) K= ? Refer to the coupled equilibria shown below. (1) Agʻ(aq) + L(aq) → AgL*(aq) K= ? (2) AgClls) = Ag"(aq) + CI (aq) K 1.83 x 10 10 %3D (3) AgCl(s) + Llaq)→ AgL*(aq) + Cl (aq) K= K¢ Kgp =23.7 0 1.30 e 11 0 1.30 e-11 0 7.72 e-12
What is Eºcell in volts? (C) || (aq) | 12 (s) || Cl₂ (g) | CI (aq) | (C) I₂ (s) + 2 e² → 2 I¯ (aq) Cl₂ (g) + 2 e → 2 C1 (aq) O +0.824 O -0.824 O -1.896 O +1.648 O -1.648 O +1.896 Eº = +0.536 V Eº = +1.360 V