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The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 - 90...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AG° at 25° for 12 H2 (g) + AgCl(s) – HCl(aq) + Ag(s) Select one: a.-23.2 kJ/mol b. 21.2 kJ/mol C.-22.2 kJ/mol d. 23.2 kJ/mol e. 22.2 kJ/mol
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard...
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant Hg2+/Hg +0.85 F = 96485 C Fe3+/Fe2+ +0.77 2Fe3+(aq) + Hg(l) → 2Fe2+(aq) + Hg2+(aq) 2. The voltaic cell described by the balanced chemical equation has a standard emf of...
For the cell: Ag 's)| H2 (9) (Р %3D 1 bar), HCI (b = 1.00 molal),...
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?
For a particular cell based on the reaction: 3 AgCl(s) + Al(s) + 3 Ag(s) +...
For a particular cell based on the reaction: 3 AgCl(s) + Al(s) + 3 Ag(s) + A13+ (aq) + 3 C (aq) E° = +1.884 V at 298K. What is the value of the equilibrium constant, K, at 298 K for the reaction? Enter your answer in exponential format (example 1.23E-4) with two decimal places and no units If you use the constants R and F in your calcłılation, use ONLY these values R = 8.31451 J/K F = 96,485...
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq)...
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: Submit Answer Retry Entire Group more group attempts remaining AH,(kJ/mol) AG® (kJ/mol) Sº (J/mol K) -238.7 -116.0 126.8 219.0 -363.0 249.0 135.1 -166.3 -110.0 -351.0 125.0 209.2 68.2 - 129.0 202.0 226.7 200.9 52.3 - 166.0 -53.0 -277.7 219.6 250.0 242.0 160.7 -13.0 -235.1 282.7 Carbon CH3OH (1) H2CO...
9. (12 pts) Answer parts a-b for the following reaction: Hos?"(aq) + 2 Ag(s) = Hg...
9. (12 pts) Answer parts a-b for the following reaction: Hos?"(aq) + 2 Ag(s) = Hg () + 2 Agt(aq) a) Calculate the equilibrium constant at 37 °C. -> 310K - С. 2 46°.. - КТК - = -8.314 (310) Ink Ecele = Fired (reduced) - Ered (oxidized) (no need to flip signs!) E = pº In QC q=1.t 1 C = 1 A-s F = 96485 C/mole e R = 8.314 J/mole K or 0.082057 L.atm/mole K PV=nRT Ered...
B. Calculate the standard entropy change for the reaction 2Na(s)+Cl2(g)?2NaCl(s) using the data from the following t...
B. Calculate the standard entropy change for the reaction
2Na(s)+Cl2(g)?2NaCl(s)
using the data from the following table:
Substance
?H?f (kJ/mol)
?G?f (kJ/mol)
S? [J/(K?mol)]
Na(s)
0.00
0.00
51.30
Cl2(g)
0.00
0.00
223.1
NaCl(s)
-411.0
-384.0
72.10
Express your answer to four significant figures and include the
appropriate units.
Part A Predict the sign of the entropy change, AS°,for each of the reaction displayed. Drag the appropriate items to their respective bins. Ag+(aq) + Cl-(aq) → AgCl(s) | | Ca(OH)2(s) →...
Consider the following analytical cell: Pt(s)|H2(g,0.10atm)|NaOH(aq,0.10M)||NaOH(aq,0.0010M)|Ag2O|Ag(s) a. If we assumed that all the reactants were under...
Consider the following analytical cell: Pt(s)|H2(g,0.10atm)|NaOH(aq,0.10M)||NaOH(aq,0.0010M)|Ag2O|Ag(s) a. If we assumed that all the reactants were under standard conditions, what is E°cell? b. What is Ecathode under the given conditions? c. What is Eanode under the given conditions? d. What is Ecell under the given conditions?
3) The other equation from today's class was the synthesis of ammonia gas. N2(g) + 3...
3) The other equation from today's class was the synthesis of ammonia gas. N2(g) + 3 H2(g) = 2 NH3(g) (8 pts) Use the thermodynamic data given in the table to answer the following questions about this reaction at standard conditions, T = 298.15 K and P = 1 atm. Substance AH (kJ/mol) S (J/mol K) N2 (g) 0 191.6 H2(g) 0 130.7 NH3(g) -46.11 192.5 A) What is AHº for this reaction? B) What is AS for this reaction?...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AG° at 25° for 12 H2 (g) + AgCl(s) – HCl(aq) + Ag(s) Select one: a.-23.2 kJ/mol b. 21.2 kJ/mol C.-22.2 kJ/mol d. 23.2 kJ/mol e. 22.2 kJ/mol
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?
For a particular cell based on the reaction: 3 AgCl(s) + Al(s) + 3 Ag(s) + A13+ (aq) + 3 C (aq) E° = +1.884 V at 298K. What is the value of the equilibrium constant, K, at 298 K for the reaction? Enter your answer in exponential format (example 1.23E-4) with two decimal places and no units If you use the constants R and F in your calcłılation, use ONLY these values R = 8.31451 J/K F = 96,485...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: Submit Answer Retry Entire Group more group attempts remaining AH,(kJ/mol) AG® (kJ/mol) Sº (J/mol K) -238.7 -116.0 126.8 219.0 -363.0 249.0 135.1 -166.3 -110.0 -351.0 125.0 209.2 68.2 - 129.0 202.0 226.7 200.9 52.3 - 166.0 -53.0 -277.7 219.6 250.0 242.0 160.7 -13.0 -235.1 282.7 Carbon CH3OH (1) H2CO...
9. (12 pts) Answer parts a-b for the following reaction: Hos?"(aq) + 2 Ag(s) = Hg () + 2 Agt(aq) a) Calculate the equilibrium constant at 37 °C. -> 310K - С. 2 46°.. - КТК - = -8.314 (310) Ink Ecele = Fired (reduced) - Ered (oxidized) (no need to flip signs!) E = pº In QC q=1.t 1 C = 1 A-s F = 96485 C/mole e R = 8.314 J/mole K or 0.082057 L.atm/mole K PV=nRT Ered...
B. Calculate the standard entropy change for the reaction
2Na(s)+Cl2(g)?2NaCl(s)
using the data from the following table:
Substance
?H?f (kJ/mol)
?G?f (kJ/mol)
S? [J/(K?mol)]
Na(s)
0.00
0.00
51.30
Cl2(g)
0.00
0.00
223.1
NaCl(s)
-411.0
-384.0
72.10
Express your answer to four significant figures and include the
appropriate units.
Part A Predict the sign of the entropy change, AS°,for each of the reaction displayed. Drag the appropriate items to their respective bins. Ag+(aq) + Cl-(aq) → AgCl(s) | | Ca(OH)2(s) →...
3) The other equation from today's class was the synthesis of ammonia gas. N2(g) + 3 H2(g) = 2 NH3(g) (8 pts) Use the thermodynamic data given in the table to answer the following questions about this reaction at standard conditions, T = 298.15 K and P = 1 atm. Substance AH (kJ/mol) S (J/mol K) N2 (g) 0 191.6 H2(g) 0 130.7 NH3(g) -46.11 192.5 A) What is AHº for this reaction? B) What is AS for this reaction?...
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