We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Question 10 3.03 pts Use the standard reduction potenital to calculate equilibrium constants for the following...
19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl (s) Ag+ (aq) +Cl- (aq) Ag+ (aq) +Ag(s) E° = 0.7996 V AgCl(s) + e - Ag(s) + CH- (aq) E° = 0.22233 V O K=5.2 x 105 spontaneous O K = 3.8 x 10"nonspontaneous K - 1.7 x 10-10 nonspontaneous
28. Use the standard reduction potenital to calculate equilibrium constants for the following reaction. H2O (1) H (aq) +OH (aq) at 298.15 K H2 (g)2H (aq) +2e 2H2O (aq) +2e - H2+ 20H (aq) A.K=1.0 x10 B. K=1.6 x10-1l C.K=1.0 x10-14 0 Define electrolvsis. E= 0V E -0.8277 V -10 spontaneous nonspontaneous nonspontaneous
27. Use the standard reduction potenital to calculate equilibrium constants for the following reaction. CdS(s) → Cd2+ (aq) +32 (aq) at 377 K Page 4 of 5 E° = -0.4030 V E° = -1.17 V Cd2+ (aq) +2e → Cd (s) CdS(s) +2e → Ca (s) +S2- (aq) A. K=1.7 x10° nonspontaneous B. K=3.1 x102 nonspontaneous C. K=1.5 x10- nonspontaneous m constants for the fol
Calculate the standard Gibbs free energy changes at 25 °C for each of the reactions shown below using the Eº values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 2 Lit(aq) + 2 I'(aq) = 2 Li(s) + 1 12(5) ° = -3.586 V AGC= X kJ/mol nonspontaneous at equilibrium spontaneous (b) 2 CO3+ (aq) + 1 Hg(0) = 2 Co2+ (aq) + 1 Hg2+(aq) ° = 0.988 V AGº =...
For the cell: Ag 's)| H2 (9) (Р %3D 1 bar), HCI (b = 1.00 molal), AgCl (s) | Ag(s) The standard cell potential was measured at different temperatures and the resulting data was fitted to a polynomial expression. The result is: E = 0.22233 - 0.0006477(T - 298.15) - 3.241 x 10-6(T - 298.15)2 Volts With T the Kelvin temperature What is the equilibrium constant for the cell reaction at 280 K?
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Fe+ (aq) + Cd(s)— 2Fe2+ (aq) + Cd²+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant AGⓇ for this reaction would be than zero. Submit Answer Retry Entire Group 6 more group attempts remaining Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu + (aq) - Cu(s)— 2Cu (aq) + Cu+...
Use the data in Appendix L to determine the equilibrium constant for the following reactions. Assume 298.15 K if no temperature is given. (a) AgCl(s) ⇌ Ag+(aq) + Cl−(aq) (b) CdS(s) ⇌ Cd2+(aq) + S2−(aq) at 377 K (c) Hg2+(aq) + 4Br−(aq) ⇌ [HgBr4 ] 2−(aq) (d) H2 O(l) ⇌ H+(aq) + OH−(aq) at 25 °C
Please show all work!
Thanks!
Calculate the equilibrium constants of the following reactions at 25°C from standard potential data (a) Sn(s) Sn+(aq)2 Sn2+(aq) 1.54e-10 (b) Sn(s) + 2 AgCl(s)SnCl2(aq) + 2 Ag(s) 2.04e18
Using the reduction potentials given, calculate the equilibrium
constant, K, at 20 degrees C for the reaction
Using the reduction potentials given, calculate the equilibrium constant, K, at 25°C for the reaction, 33 3+ Ag (aa) t Fe(a)Ag) Fe (aq) +0.77 V +0.80 V A Ag+(aq) + e- ← a. 1.66 b. 6.4 c. 3.2 d. 6.1 x 10-4 e. 1.6 x 104 Rank the following compounds according to increasing solubility in water. K” is a less than sign) 34...
Question 8 3.03 pts Based on the following reduction potential data, what is the AGºran for the following electrochemical cell reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)? Eres -0.763 V for Zn2+ (aq) + 2e - Zn(s) Ered = +0.340 V for Cu2+(aq) + 2e - Cu(s) O +106 kJ/mol O-106 kJ/mol -213 kJ/mol