The change of E°(Ag+ | Ag) with temperature is –0.00100 V K–1. If you determined E°(Ag+...
The change of E°(Ag+ | Ag) with temperature is –0.00100 V K–1. If you determined E°(Ag+ | Ag) to be 0.805 V at 22.0 °C, what would the value be, once corrected for temperature, at 25.0 °C?
Homework Answers
Hence the value for the cell potential at 25.0 C will be equal to 0.802 V
Note - Post any doubts/queries in comments section.
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The change of E°(Ag+ | Ag) with temperature is –0.00100 V K–1.
If you determined E°(Ag+...
At what temperature will it change between spontaneous and nonspontaneous? e. What is K for the...
At what temperature will it change between spontaneous and nonspontaneous? e. What is K for the reaction? Write the equilibrium constant expression (K) for the following balanced reactions. Indicate the type of equilibrium constant (Kc, Ka, Kb, K_sp, Kf etc) a. PbAgAsS_3(s)+H_2 O(1) = Pb^+ 2 + Ag* + As^+3 + 3 s^-2 CO_2 (aq) + H_2 O(1) H_2 CO_3 (aq) How will each of the following changes affect the equilibrium mixture? NH_4HS(s) NH_3(g), + H_2 S(g) Rxn is endothermic...
1. What would be the effect on the enthalpy change determined if the temperature probe read...
1. What would be the effect on the enthalpy change determined if the temperature probe read 1.0°C lower than the true temperature? Explain. (2 pts)
Z. Consider the following data: E(Ag O/Ag- +1.36 V; EAg g")-+1.98 V; E(Ag/Ag)-+0.80 V; E (Ag.S/AgH2S)--0.69...
Z. Consider the following data: E(Ag O/Ag- +1.36 V; EAg g")-+1.98 V; E(Ag/Ag)-+0.80 V; E (Ag.S/AgH2S)--0.69 v (a) Which of the five species (Ag S, Ag:O, Ag g,Ag) is the strongest oxidizer and which one should be the easiest to oxidize? (b) The standard hydrogen electrode is connected with an electrode made of silver and containing Ag ions in water as shown below: Ag Which of the electrodes is the cathode and which is the anode? Which way the electrons...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standar...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standard potential for the cell reaction for 2 Ag + H2 (g)-2 Ag+2H +0.80 V b. a. +0.40 V +0.12 V d. c. -0.12 v none of these e. 40. Given: Fe (s) + 2 Ag' (aq) Fe (ag)+ 2 Ag (s) with E ell -1.24 V What is the...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
salt bridge Pb2+2 e Eo0.13 V Pb (s) Ag1 e o = 0.80 V Ag (s)...
salt bridge Pb2+2 e Eo0.13 V Pb (s) Ag1 e o = 0.80 V Ag (s) What is the voltage, at 298 K, of this voltaic cell starting with the following non-standard concentrations: [Pb2+1 (aq) 0.063 M [Ag (aq) 0.61 M Use the Nernst equation: E=E- (RT/nF) In Q First calculate the value of Q, and enter it into the first answer box. Q is dimensionless. Then calculate E, the non-standard cell potential, and enter its value into the second...
QUESTION 25 Match the following Q=K Q<k Q>K A. AG > AG B.DGO C equilibrium D....
QUESTION 25 Match the following Q=K Q<k Q>K A. AG > AG B.DGO C equilibrium D. AGO E. standard state F. AG AG G.K=0 - Q = 1 Q> Q< 1 QUESTION 15 For a reaction at equilibrium, AS univ=0. True False QUESTION 16 As a chemical reaction proceeds toward equilibrium, the free energy of the system decreases. True False QUESTION 17 For a given reaction, a change in the pressure may result in a change in the sign of...
Given: C+++ (aq) +3e" = Cr(s);E°=-0.74V Ag+ (aq) +e Ag(s); E° = 0.80 V What is...
Given: C+++ (aq) +3e" = Cr(s);E°=-0.74V Ag+ (aq) +e Ag(s); E° = 0.80 V What is the cell potential at 25°C for the following cell? Cr(s) | Cr3+(0.010 M) || Ag+(0.00025 M) | Ag(s) a) 1.71 V b) 1.51 V O c) 0.95 V d) 2.09 V e) 1.37 V
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) Substance CO(NH2)2(aq) H2O(1) CO2(g) NH AH° (kJ/mol) -391.2 -285.9 -393.5 -46.19...
At what temperature will it change between spontaneous and nonspontaneous? e. What is K for the reaction? Write the equilibrium constant expression (K) for the following balanced reactions. Indicate the type of equilibrium constant (Kc, Ka, Kb, K_sp, Kf etc) a. PbAgAsS_3(s)+H_2 O(1) = Pb^+ 2 + Ag* + As^+3 + 3 s^-2 CO_2 (aq) + H_2 O(1) H_2 CO_3 (aq) How will each of the following changes affect the equilibrium mixture? NH_4HS(s) NH_3(g), + H_2 S(g) Rxn is endothermic...
1. What would be the effect on the enthalpy change determined if the temperature probe read 1.0°C lower than the true temperature? Explain. (2 pts)
Z. Consider the following data: E(Ag O/Ag- +1.36 V; EAg g")-+1.98 V; E(Ag/Ag)-+0.80 V; E (Ag.S/AgH2S)--0.69 v (a) Which of the five species (Ag S, Ag:O, Ag g,Ag) is the strongest oxidizer and which one should be the easiest to oxidize? (b) The standard hydrogen electrode is connected with an electrode made of silver and containing Ag ions in water as shown below: Ag Which of the electrodes is the cathode and which is the anode? Which way the electrons...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standard potential for the cell reaction for 2 Ag + H2 (g)-2 Ag+2H +0.80 V b. a. +0.40 V +0.12 V d. c. -0.12 v none of these e. 40. Given: Fe (s) + 2 Ag' (aq) Fe (ag)+ 2 Ag (s) with E ell -1.24 V What is the...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
salt bridge Pb2+2 e Eo0.13 V Pb (s) Ag1 e o = 0.80 V Ag (s) What is the voltage, at 298 K, of this voltaic cell starting with the following non-standard concentrations: [Pb2+1 (aq) 0.063 M [Ag (aq) 0.61 M Use the Nernst equation: E=E- (RT/nF) In Q First calculate the value of Q, and enter it into the first answer box. Q is dimensionless. Then calculate E, the non-standard cell potential, and enter its value into the second...
QUESTION 25 Match the following Q=K Q<k Q>K A. AG > AG B.DGO C equilibrium D. AGO E. standard state F. AG AG G.K=0 - Q = 1 Q> Q< 1 QUESTION 15 For a reaction at equilibrium, AS univ=0. True False QUESTION 16 As a chemical reaction proceeds toward equilibrium, the free energy of the system decreases. True False QUESTION 17 For a given reaction, a change in the pressure may result in a change in the sign of...
Given: C+++ (aq) +3e" = Cr(s);E°=-0.74V Ag+ (aq) +e Ag(s); E° = 0.80 V What is the cell potential at 25°C for the following cell? Cr(s) | Cr3+(0.010 M) || Ag+(0.00025 M) | Ag(s) a) 1.71 V b) 1.51 V O c) 0.95 V d) 2.09 V e) 1.37 V
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) Substance CO(NH2)2(aq) H2O(1) CO2(g) NH AH° (kJ/mol) -391.2 -285.9 -393.5 -46.19...
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