librium constant for the reaction Sr(s) + Mg (a)+ Mgo) is 2.69 × 1012 at 25°C....
The equilibrium constant for the reaction Sr(s) + Mg2+(aq) ⇌ Sr2+(aq) + Mg(s) is 3.69 × 1017 at 25°C. Calculate E o for a cell made up of Sr / Sr2+ and Mg / Mg2+ half-cells. V
1A) the equilibrium constant of reaction Sr(s)+Mg24(ac)---><--- Sr24(ac)+Mg(s) is 2.69X1012 at 25º C calculate the Eº of the cell formed by the half cells Sr / Sr2 + and Mg / Mg2 + R= 8.314 J/k -mol F= 96500 J/V- mol 1B) Calculate the standard emf of a cell using the Ag / Ag1 + and Al / Al3 + half-cell reactions. answers A)0.86 V B)2.46 V C)-1.86 V D)-0.86 V E cell AGⓇ =-nFEcell Ecell = F Ink AG°...
If the equilibrium constant (Keq) equals 6.09x1012 for the following reaction between strontium and magnesium: Sr(s) + Mg2+(aq)<==> Sr2+(aq) + Mg(s) Calculate Eo for a strontium=magnesium battery. Enter in volts.
Consider the following reaction and its AGⓇ at 25 °C. Mg(s) + Ni2+(aq) — Mg2+(aq) + Ni(s) AG° = -408.0 kJ/mol Calculate the standard cell potential, Ecell, for the reaction. Fo Celi Calculate the equilibrium constant, K, for the reaction.
(a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: Ca + Sr2+ → Ca2+ + Sr (b) What is the value of E if the concentration of Sr2+ is 8.17 x 10-5 and the concentration of Ca2+ is 8.48 x 10-6? (c) If E = 0.28 V and Sr2+ = 0.10 M, what is the concentration of...
Given the data in Appendix B in the textbook, calculate Kp at 25 ∘C for the reaction MgCO3(s)⇌MgO(s)+CO2(g) lnK = -19.45
Calculate the standard enthalpy change for the following reaction at 25 °C. MgCl, (s)+H,O)MgO(s)+2 HCI(g) AH; values can be found in this table of thermodynamic values. AH= kJ/mol
14. Calculate Ecal and the equilibrium constant, K, for the following reaction at 25°C. Cd(s) + Fe (aq) C&" (aq) + Fe(s) E-0.0592 Log K n 15. Calculate the cell potential, E, for the reaction below at 25 C if [H'] = 1.0 M, [Zn**] -0.0010 M, and Pre: -0.10 atm. (Hint. Find Ece and then use the relationship EE-0.0592 log Q) n Zn(s) +21 -2H(aq) ® Zn"(aq) +H-8) 16. Balance the following reactions MnO + Br® MnO+ Br, (in...
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s)+3 Mg2+(aq) A) 1.1 x 1072 B) 8.9 x 10-73 C) 1.1 x 10-72 D) 1.0 x 1024 E) 4.6 x 1031 2 Al3+(aq) +3 Mg(s)
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo