![Given Shaw +6f → [ShF6] 2- complete cell Half cell reactins- [Snp6]?+e- →Sno tofaq E°N) = reaction shtetas tte. ~> Sn(s). EW](http://img.homeworklib.com/questions/d2db18a0-3fe7-11eb-a518-a7522710e6b8.png?x-oss-process=image/resize,w_560)
D Question 39 1 pts Given the information below, calculate the equilibrium constant of the reaction:...
show and explain work please
6. Calculate the equilibrium constant at 25°C for the following reaction: Cd(s) + Sn** (aq) → Cd²+ (aq) + Sn(s) K = 6.3 x 108
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction? (R= 8.314 J/K.mol, F = 96,500 C-moll) Sn2+ (aq) + Fe(s) Sn(s) + Fe2+(aq) E cell = 0.35 V O 7.1 x 10-11 1.2 x 1010 1.2 x 105 8.6 x 10- 2.3 1023 QUESTION 30 A chemist adds substance A and B to a reaction flask and allows equilibrium to establish A+B=CKc= 1.5 x 10-25 Which of the following describe the contents of...
Question 9 1 pts What is the reaction quotient (Q) for the equilibrium TISCN(s) Tit(aq) + SCN*(aq) when 0.1837 L of 1.265 x 10-2 M Tit is combined with 0.1335 L of 4.216 x 10-4 M SCN" in the presence of an excess of TISCN(s)? O 1.3 x 10-6 5.333 x 10- 1.308 x 10-6 4.123 x 10-6 0 5.366 x 10-6
Question 10 1 pts For the reaction Cu2S(s) =2Cu* (aq) +52-(aq), the equilibrium concentrations are as follows: (Cut) = 1.0~10-5 M, [52-)- 10 x 10-2 M. The equilibrium constant is: 1.0 x 107 1.0 x 10-12 O 1.0x 10 % 1.0 x 107.
Question 8 1 pts Which equilibrium constant represents a reaction that favors the reactants to the greatest extent? O keq = 1.0 x 10-3 o Keq=100 O keq = 1.0 x 10-18 Keq = 1.0 x 10 Previous
Question 10 3.03 pts Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl(s) Ag+ (aq) +CH(aq) Ag+ (aq) +eAg(s) E° =0.7996 VAgCl(s) + e - Ag(s) + CH(aq) E° = 0.22233 V OK-5.2 x 10% spontaneous OK=3.8 x 10nonspontaneous N O K=1.7 x 10-10 nonspontaneous
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
D Question 4 1 pts The reaction shown is at equilibrium. If a student adds more X to the system, what happens immediately (at that instant) to Q and K? X Y Z Both decrease Both increase O Qgets larger and gets smaller K gets larger and gets smaller Kremains constant and increases Kremains constant and a decreases 1 pts Question 5 You have a saturated solution of Ca(OH)2 in a flask, meaning there is some solid CaOH)2 sitting at...