For the following questions: a)Calculate ??????for the spontaneous reaction b)Write the overall cell equation c)Write the...
For the following questions:
a)Calculate ??????for the spontaneous reaction
b)Write the overall cell equation
c)Write the cell notation for the cell
d)Calculate ???
e)Calculate ?????where non-standard conditions are stated
1)cell is made from the ??3+,(??,0.10?)|??and the ???4-(??,0.25?)|??2+,(??,1.50?)half cells, where pH is 1.67 at 298 K(no need to calculate ???for this Q)
2)A cell is made from the ??|??+,(??,0.010?)and the ???4-(??,2.0?)|???2half cells, where pH is 0 at 298 K(no need to calculate ???for this Q)
Homework Answers
![id) en keqb = tftice cell NRT - keqb=54.399 2 +965008 1.55 1578.3148 298 ces Ecell- E cell 0.0591 log [f234 [ant 2] [ho] [H](http://img.homeworklib.com/questions/061253c0-85f6-11eb-9414-8b5b5b31edc0.png?x-oss-process=image/resize,w_560)
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For the following questions:
a)Calculate ??????for the spontaneous reaction
b)Write the overall cell equation
c)Write the...
i am confuses how to calculate Ecell where non-standard condition for this question For the following...
i am confuses how to calculate Ecell where non-standard
condition for this question
For the following questions: a) Calculate Ece for the spontaneous reaction b) Write the overall cell equation c) Write the cell notation for the cell d) Calculate Keg e) Calculate E cell where non-standard conditions are stated 5) A cell is made from the Sn|Sn2+(aq, 2.00 M) and the C10,(g, 0.100 atm|C10, (aq, 2.00 M) half cells at 298 K
Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is ...
Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answerNV here. Be sure your answer has the correct number of significant digits A chemist designs a galvanic cell that uses these two half-reactions half-reaction standard reduction potential Eed+1.51...
8) (16 pts) For the following cell diagram, Cr20,2 (aq)IC3+(aq) Cl-(aq)ICl2(8) A. Write the reduction and...
8) (16 pts) For the following cell diagram, Cr20,2 (aq)IC3+(aq) Cl-(aq)ICl2(8) A. Write the reduction and oxidation half reactions, balance the equation in acidic condition. Combined reaction: B. Determine the standard cell potential E cell Is the reaction spontaneous? C. Once the two hal reaction quotient and Nernst' equation. f cells are connected and allowed to discharge for a while, discuss how cell potential changes F. Calculate the standard free energy change for this reaction. G. Determine the equilibrium constant...
(14-17) (a) Write the line notation for the following cell. reaction. (c) From you sometimes led...
(14-17) (a) Write the line notation for the following cell. reaction. (c) From you sometimes led (d) Extra cred manganese reactions in 2M HBr(aq, 0.10 M) Mn Use the me manganese net cell rea The m: (4). For ea ber of mol tion is AG in Append electroni Br (0) Al(NO )3(aq, 0.010 M) (b) Calculate the potential of each half-cell and the cell voltage, E. In which direction will electrons flow through the circuit? Write the spontaneous net cell...
14. Determine the standard cell potential and the cell potential under the stated conditions for the...
14. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at 298.15 K. a) Hg(l) + S2-(ag, 0.10 M) + 2Ag+(ag, 0.25 M) → 2Ag(s) + HgS(s) \ (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half-cell consisting of a nickel electrode in 0.25 M...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State wheth...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
Need help with number 3 please. 3. A voltaic cell is buiit from the half-cells described...
Need help with number 3 please.
3. A voltaic cell is buiit from the half-cells described below Half-cell 1: Copper electrode it 0.10 M Cu solution Half-cell 2: Platinum electrode in a solution that is 0.050 M Fe and 0,050 M Fe a. Weite the line notation for the cell. b. Draw a diagram of the cell. Label the anode and cathode, Label the direction of electron flow thorough the wire and ion flow through the salt bridge. c. Write...
Voltaic cells chemistry please help with A-C, H and I. 3. A voltaic cell is built...
Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built from two half-cells using the reduction reactions given below: Sn 2(aq) → Sn(s); Eredn = -0.14 V Cr20;2(aq) → Cr+ (aq) Eredin = 1.33 V a) Write the balanced cathode half reaction in acidic medium: (show work step by step and box your answer) b) Write the balanced anode half reaction and box your answer: c) Write the balanced overall cell reaction and box...
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram...
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Zinc and iron electrodes, aqueous zinc nitrate, aqueous iron (III) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e- → Fe (s) E°= -0.040 V Ag+(aq) + e- → Ag(s) E°= 0.795 V a. Identify the electrodes as Anode or Cathode. Write the correct metal for each assuming the reactions are spontaneous b. Show the direction of the electron...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
i am confuses how to calculate Ecell where non-standard
condition for this question
For the following questions: a) Calculate Ece for the spontaneous reaction b) Write the overall cell equation c) Write the cell notation for the cell d) Calculate Keg e) Calculate E cell where non-standard conditions are stated 5) A cell is made from the Sn|Sn2+(aq, 2.00 M) and the C10,(g, 0.100 atm|C10, (aq, 2.00 M) half cells at 298 K
Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answerNV here. Be sure your answer has the correct number of significant digits A chemist designs a galvanic cell that uses these two half-reactions half-reaction standard reduction potential Eed+1.51...
8) (16 pts) For the following cell diagram, Cr20,2 (aq)IC3+(aq) Cl-(aq)ICl2(8) A. Write the reduction and oxidation half reactions, balance the equation in acidic condition. Combined reaction: B. Determine the standard cell potential E cell Is the reaction spontaneous? C. Once the two hal reaction quotient and Nernst' equation. f cells are connected and allowed to discharge for a while, discuss how cell potential changes F. Calculate the standard free energy change for this reaction. G. Determine the equilibrium constant...
(14-17) (a) Write the line notation for the following cell. reaction. (c) From you sometimes led (d) Extra cred manganese reactions in 2M HBr(aq, 0.10 M) Mn Use the me manganese net cell rea The m: (4). For ea ber of mol tion is AG in Append electroni Br (0) Al(NO )3(aq, 0.010 M) (b) Calculate the potential of each half-cell and the cell voltage, E. In which direction will electrons flow through the circuit? Write the spontaneous net cell...
14. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at 298.15 K. a) Hg(l) + S2-(ag, 0.10 M) + 2Ag+(ag, 0.25 M) → 2Ag(s) + HgS(s) \ (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half-cell consisting of a nickel electrode in 0.25 M...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
Need help with number 3 please.
3. A voltaic cell is buiit from the half-cells described below Half-cell 1: Copper electrode it 0.10 M Cu solution Half-cell 2: Platinum electrode in a solution that is 0.050 M Fe and 0,050 M Fe a. Weite the line notation for the cell. b. Draw a diagram of the cell. Label the anode and cathode, Label the direction of electron flow thorough the wire and ion flow through the salt bridge. c. Write...
Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built from two half-cells using the reduction reactions given below: Sn 2(aq) → Sn(s); Eredn = -0.14 V Cr20;2(aq) → Cr+ (aq) Eredin = 1.33 V a) Write the balanced cathode half reaction in acidic medium: (show work step by step and box your answer) b) Write the balanced anode half reaction and box your answer: c) Write the balanced overall cell reaction and box...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
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