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(13)(8 pts) Consider the following reaction at room temperature: Co(s) + Fe2+(aq, 1.94M) → 2 Co2+(aq,...
Consider the following reaction and its AG at 25.00 °C. Fe2+ (aq) + Zn(s) Fe(s) +...
Consider the following reaction and its AG at 25.00 °C. Fe2+ (aq) + Zn(s) Fe(s) + Zn2+ (aq) AG = -60.73 kJ/mol Calculate the standard cell potential, E , for the reaction. Ecell Calculate the equilibrium constant, K, for the reaction.
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell =...
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell = 0.78 V If [Cu2+] = 0.3 M, what [Fe2+] is needed so that Ecell = 0.76 V 2- Calculate the Eocell for the following redox reaction: Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s)
Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) +Zn(s)Fe(s)+ Zn2 (aq) AG=-60.73 kJ/mol...
Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) +Zn(s)Fe(s)+ Zn2 (aq) AG=-60.73 kJ/mol Calculate the standard cell potential, E for the reaction. V Ell Calculate the equilibrium constant, K, for the reaction. K =
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) +...
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E o (Fe2+ / Fe) = −0.4400 V, E o (Cd2+ / Cd) = −0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.60 M and [Cd2+] = 0.010 M. E =____ V Will the reaction occur spontaneously at these conditions? yes no cannot predict
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) +...
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E° (Fe2+ / Fe) =-0.4400 V, Eº (Cd2+ / Cd) = -0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.85 M and [Cd2+] = 0.010 M. E= Lv Will the reaction occur spontaneously at these conditions? o o yes no cannot predict o
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) +...
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) e°(Fe2+ / Fe) = -0.4400 V, Eº (Cd2+ / Ca) = -0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+1 0.75 M and Ca2+] = 0.010 M. E- L v Will the reaction occur spontaneously at these conditions? O yes no cannot predict
answ 10. 11, 12 xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Wh...
answ 10. 11, 12
xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Which of the of the following changes in condition will cause the equilibrium to shift to the right? (3 pts) (A) add Fe (B) removeCO ( C M CO (D) raise the temperature . Calculate the equilibrium copcentrations of land lat 700 K in a vessel that contains initial concentration of HI -0.36 M. The equilibrium...
Consider the following unbalanced equation. H1+(aq) + Fe(s) → H2(g) + Fe2+ (aq) (a) What are...
Consider the following unbalanced equation. H1+(aq) + Fe(s) → H2(g) + Fe2+ (aq) (a) What are the following standard voltages? Includeţthe sign. Change the sign as allowed by the data in the table. standard oxidation potential for the oxidation half-cell .00 X V reduction potential for the reduction half-cell .44 X V potential for the entire cell (b) Select all that apply for the reaction under standard conditions. Hl+ is the substance being oxidized. Fe is the substance being oxidized....
1. What is the value (in V) of Eocell for the following reaction? Co2+ (aq) +...
1. What is the value (in V) of Eocell for the following reaction? Co2+ (aq) + Be (s) → Co (s) + Be2+ (aq) 2.What is Eocell (in V) for a redox reaction where one electron is transferred with an equilibrium constant (K) of 1.44 x 10-14? 3.Consider the following reaction: Cu2+ (aq) + Pb (s) → Cu (s) + Pb2+ (aq) What will be Ecell for this reaction (in V) when [Cu2+] = 0.500 M and [Pb2+] = 0.0350...
Pt(s) + Fe2+ (aq) - P+2+ (aq) + Fe(s) [Fe2+] = 0.0083 M [P+2+] = 0.030...
Pt(s) + Fe2+ (aq) - P+2+ (aq) + Fe(s) [Fe2+] = 0.0083 M [P+2+] = 0.030 M The cell is not spontaneous. O spontaneous. Cu(s) + 2 Ag+ (aq) Cu2+ (aq) + 2 Ag(s) (Cu²+] = 0.013 M [Ag+] = 0.013 M The cell is O not spontaneous O spontaneous. Co2+ (aq) + T18+ (aq) [Co2+] = 0.060 M (T3+1 = 0.0060 M Co + (aq) + Ti”+ (aq) Co+] = 0.050 M [Ti?+] = 0.0115 M E-L v The...
Consider the following reaction and its AG at 25.00 °C. Fe2+ (aq) + Zn(s) Fe(s) + Zn2+ (aq) AG = -60.73 kJ/mol Calculate the standard cell potential, E , for the reaction. Ecell Calculate the equilibrium constant, K, for the reaction.
Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) +Zn(s)Fe(s)+ Zn2 (aq) AG=-60.73 kJ/mol Calculate the standard cell potential, E for the reaction. V Ell Calculate the equilibrium constant, K, for the reaction. K =
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E° (Fe2+ / Fe) =-0.4400 V, Eº (Cd2+ / Cd) = -0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.85 M and [Cd2+] = 0.010 M. E= Lv Will the reaction occur spontaneously at these conditions? o o yes no cannot predict o
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) e°(Fe2+ / Fe) = -0.4400 V, Eº (Cd2+ / Ca) = -0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+1 0.75 M and Ca2+] = 0.010 M. E- L v Will the reaction occur spontaneously at these conditions? O yes no cannot predict
answ 10. 11, 12
xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Which of the of the following changes in condition will cause the equilibrium to shift to the right? (3 pts) (A) add Fe (B) removeCO ( C M CO (D) raise the temperature . Calculate the equilibrium copcentrations of land lat 700 K in a vessel that contains initial concentration of HI -0.36 M. The equilibrium...
Consider the following unbalanced equation. H1+(aq) + Fe(s) → H2(g) + Fe2+ (aq) (a) What are the following standard voltages? Includeţthe sign. Change the sign as allowed by the data in the table. standard oxidation potential for the oxidation half-cell .00 X V reduction potential for the reduction half-cell .44 X V potential for the entire cell (b) Select all that apply for the reaction under standard conditions. Hl+ is the substance being oxidized. Fe is the substance being oxidized....
Pt(s) + Fe2+ (aq) - P+2+ (aq) + Fe(s) [Fe2+] = 0.0083 M [P+2+] = 0.030 M The cell is not spontaneous. O spontaneous. Cu(s) + 2 Ag+ (aq) Cu2+ (aq) + 2 Ag(s) (Cu²+] = 0.013 M [Ag+] = 0.013 M The cell is O not spontaneous O spontaneous. Co2+ (aq) + T18+ (aq) [Co2+] = 0.060 M (T3+1 = 0.0060 M Co + (aq) + Ti”+ (aq) Co+] = 0.050 M [Ti?+] = 0.0115 M E-L v The...
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