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16. Calculate the equilibrium constant, Ksp, at 25 °C for the reaction: AgCl(s) = Ag+ (aq) + Cl(aq) given the table of standard free energies of formation. AgCI Agt Cl AGE° (kJ/mol) -109.8 77.1 -131.3 a) 0.0 b) 5.6 x 109 c) 1.7 x 10-29 d) 0.98 e) 1.8 x 10-10

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Related questions

± Cell Potential and Equilibrium
18 of 28
Constants | Periodic Table
The equilibrium constant, K, for a redox reaction is related to the standard potential, E?, by the equation
lnK=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
Sn4+(aq)+4e??Sn(s) 0.15
2H+(aq)+2e??H2(g) 0
Ni2+(aq)+2e??Ni(s) ?0.26
Fe2+(aq)+2e??Fe(s) ?0.45
Zn2+(aq)+2e??Zn(s) ?0.76
Al3+(aq)+3e??Al(s) ?1.66
Mg2+(aq)+2e??Mg(s) ?2.37

Part A Part complete
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ?C) for the following reaction:
Fe(s)+Ni2+(aq)?Fe2+(aq)+Ni(s)
Express your answer numerically.
View Available Hint(s)
K = 2.68×10^6 Correct
When E?>0 and K>1 the reaction favors the products.

Part B
Calculate the standard cell potential (E?) for the reaction
X(s)+Y+(aq)?X+(aq)+Y(s)
if K = 7.87×10?3.

Express your answer to three significant figures and include the appropriate units.

E? = ?

1. Calculate the standard change in free energy ?G? (kJ) at 298 K for the reaction C2H4(G)+3o2(G) --> 2CO2(G)+2H2O(G)

a -1310 b. +1180 c. -691 d. +1310 e. -1180

2. The value of E?cell for the reaction 2Cr3+(aq)+6Hg(l) --> 2Cr(s)+3Hg22+(aq) is 1.59 V. Calculate the ?G? (kJ) for the reaction.

a. -921 b. -153 c. -767 d. -460 e. -307

3. What is the value of the equilibrium constant for the cell reaction below at 25 deg C? E?cell­=0.61V 2Cr(s)+3Pb2+(aq) <---> 3Pb(s)+2Cr3+(aq)

a. 8.2*10^30 b. 6.7*10^61 c. 9.9*10^99 d. 4.1*10^20 e. 3.3*10^51

4. Which one of the following is not a redox reaction?

a. Na6FeCl8(s)+2Na(l) ---> 8NaCl(s)+Fe(s)

b. Al(OH)3 (aq)+3H+ ---> Al3+(aq)+3H2O(l)

c. CuCl2(aq)+Ni(s) ---> Cu(s)+NiCl2(aq)

d. C6H12O6(s)+6O2(g) ---> 6CO2+6H2O(l)

e. CO­2(g)+H2(g) ---> CO(g)+ H2O(g)­­­­­­­­

5. A voltaic cell consists of a Zn/ZN2+ electrode and a Fe/Fe2+ electrode. If [ZN2+] = 0.005M and if [Fe2+] = .0500 M , what is Ecell?

a. .76 b. 0.25 c. 0.45 d. 0.31 e. 0.37

6. The formation constant for the reaction Ag+ (aq)+2NH3(aq) <----> Ag(NH3)2+(aq) is K=1.7*107 at 25 deg C. What is the ?G?(kJ/mol) at this temperature?

a. -23 b. -18 c. -3.5 d. -1.5 e. -41

7. Nitric oxide reacts with chlorine to form NOCL. What is the free energy (kJ) of the reaction at 277 deg C?

a. +144 b.. -41.0 c. -10.3 d. -22.2 e. +41.0

8. Estimate the boiling point (deg C) of phosphoric Acid.

H3PO4(s) <----> H­3PO4(l)

?H?f kJ/mol -1279 - -127.17

?G?f kJ/mol -1119 - 1123.6

?S?f J/(k mol) 110.5 - 150.8

a. 42 b. 181 c. 315 d. -92 e. 305

9. Calculate the equilibrium constant, K, for the following reaction at 25?C:

CH4(g)+2H2O(g) <---> Ã CO2(g)+4H2(g) ?G?= -113.6 kJ (please show ICE chart and explain process)

a. 8.2x1019 b. 0.58 c. 0.96 d. 1.4x10-46 e. 1.2x10-20

10. Which of the following results in a decrease in the entropy of the system?

a. O2(g), 300K --> O2(g), 400K b. H2O(s) --> H2O(l) c. N2(g) --> N2(aq) d. NH3(l) --> NH3(g)

e. 2H2O2(g) ---> 2H2O(g)+O2(g)

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