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Calculate AG for the reaction below if E° = -2.123 V. Also indicate if the cell...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an el...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
3.Consider a galvanic cell based on the reaction. Assume theses reactions are carried out in acidic...
3.Consider a galvanic cell based on the reaction. Assume theses reactions are carried out in acidic media and that all concentrations are 1M and that all partial pressures are 1 atm. a) MnO4 (ag)+ CIO3 (ag) CIO4 (ag) + Mn (aq) b) Cr (aq+ Cl2(ag) Cr O2 +CI (aq) (aq) For each the above overall reactions, answer thee following questions. identify the cathode and anode. b. Give the overall balanced equation. How many electrons are transferred? a. c. d. Calculate...
For the balanced net redox reaction below, determine its standard cell potential (in V) at 25°C...
For the balanced net redox reaction below, determine its standard cell potential (in V) at 25°C and whether the reaction is spontaneous at standard conditions. 3Ni2+(aq) + 2Cr(s) +3Ni(s) + 2Cr3+ (aq) -0.487, spontaneous 0.487 V, nonspontaneous -0.487, nonspontaneous 0.487 V, spontaneous
please help wirh D E and F AG for the reaction = 13. (50) For the...
please help wirh D E and F
AG for the reaction = 13. (50) For the reaction in base. H2O2(aq) + ClO2(aq) → CO2 (aq) + O2(g) - to ges tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode, components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly, On the lines under each half-cell, write the balanced...
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction...
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction and its standard cell potential (in V) at 25°C for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction (please provide)= standard cell potential V= Is the reaction spontaneous at standard conditions?
Use the tables on the next page and your initials to generate a ‘cell diagram’ where...
Use the tables on the next page and your
initials to generate a ‘cell diagram’ where the first
reaction (first initial) is the anode and the second reaction
(second initial) is the cathode and determine whether the reaction
is spontaneous. For gasses, assume an inert Platinum electrode.
First Initial: K . Last Initial: D
Rxn K --> anode (off table, as a reduction) Zn
+2(aq) + 2 e- -----> Zn(s)
Rxn S --> cathode (off table) ...
the next question prevents changes to this answer. Question 24 Calculate the AG* for a reaction...
the next question prevents changes to this answer. Question 24 Calculate the AG* for a reaction at 455K at a Keq = 1,44*104. Is the reaction endergonic or exergonic. OA.-36.2 kJ/mol; endergonic 13.6 kj/mol endergonic OB Ос. 13.6 kJ/mot exergonic OD -36.2 k/mot exergonic Moving to the next question prevents changes to this answer. IMG_3716.jpg IMG_3711:09 o 99 hp 6 7 8 F E Y Т. U
number 13 a-i please AG for the reaction - 13. (50) For the reaction in base,...
number 13 a-i please
AG for the reaction - 13. (50) For the reaction in base, H.O.(aq) + CIO.(aq) → CIO, (aq) + O2(g) to gas tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly. On the lines under each half-cell, write the balanced half-cell reaction which will...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
3.Consider a galvanic cell based on the reaction. Assume theses reactions are carried out in acidic media and that all concentrations are 1M and that all partial pressures are 1 atm. a) MnO4 (ag)+ CIO3 (ag) CIO4 (ag) + Mn (aq) b) Cr (aq+ Cl2(ag) Cr O2 +CI (aq) (aq) For each the above overall reactions, answer thee following questions. identify the cathode and anode. b. Give the overall balanced equation. How many electrons are transferred? a. c. d. Calculate...
For the balanced net redox reaction below, determine its standard cell potential (in V) at 25°C and whether the reaction is spontaneous at standard conditions. 3Ni2+(aq) + 2Cr(s) +3Ni(s) + 2Cr3+ (aq) -0.487, spontaneous 0.487 V, nonspontaneous -0.487, nonspontaneous 0.487 V, spontaneous
please help wirh D E and F
AG for the reaction = 13. (50) For the reaction in base. H2O2(aq) + ClO2(aq) → CO2 (aq) + O2(g) - to ges tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode, components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly, On the lines under each half-cell, write the balanced...
Use the tables on the next page and your
initials to generate a ‘cell diagram’ where the first
reaction (first initial) is the anode and the second reaction
(second initial) is the cathode and determine whether the reaction
is spontaneous. For gasses, assume an inert Platinum electrode.
First Initial: K . Last Initial: D
Rxn K --> anode (off table, as a reduction) Zn
+2(aq) + 2 e- -----> Zn(s)
Rxn S --> cathode (off table) ...
the next question prevents changes to this answer. Question 24 Calculate the AG* for a reaction at 455K at a Keq = 1,44*104. Is the reaction endergonic or exergonic. OA.-36.2 kJ/mol; endergonic 13.6 kj/mol endergonic OB Ос. 13.6 kJ/mot exergonic OD -36.2 k/mot exergonic Moving to the next question prevents changes to this answer. IMG_3716.jpg IMG_3711:09 o 99 hp 6 7 8 F E Y Т. U
number 13 a-i please
AG for the reaction - 13. (50) For the reaction in base, H.O.(aq) + CIO.(aq) → CIO, (aq) + O2(g) to gas tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly. On the lines under each half-cell, write the balanced half-cell reaction which will...
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