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8. Which of the following statements about the voltaic cell shown below is INCORRECT? Cr(s)|Cr* (aq)||C1,(8)|CI...
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr...
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr Cr3+ half cell and the cathode is a SnSn2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: + + In the external...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M)...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)
3. The following redox couple was used in the construction of a voltaic cell. (All ions...
3. The following redox couple was used in the construction of a voltaic cell. (All ions are in aqueous solution and you ned to decide which haif resetion wil e in he cahode side and wh the cathode side and which in the anode side.) For the cell: . Make a sketch of the cell labeling anode, cathode, salt bridge (using KNOs), direction of electron flow, oxidation half ell, reduction half cell, charge of the anode, charge of the cathode,...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s)...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
20) 20) Which of the following statements concerning a voltaic cell is FALSE A) At the...
20) 20) Which of the following statements concerning a voltaic cell is FALSE A) At the anode a substance will lose electrons. B) A voltaic cell uses an oxidation-reduction reaction to produce electrical energy. C) The oxidation half reaction occurs at the cathode. D) The cell consists of two half cells. E) The anode and the cathode are separated by a salt bridge. - 21) The fluoride rinse in dental offices usually contains sodium fluoride, Sodium fluoride 2 1 can...
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)||...
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq)|Cu(s) (a) The oxidation half-reaction is clearly Zn(s) ® Zn** (aq) + 2 e. (b) The oxidation half-reaction is clearly Zn() Zn" (aq) +le. (C) The oxidation half-reaction could not be anything other than Cu(s) ® Cu (aq) +2 e. (d) It is obvious that the oxidation half-reaction is Zn(s) ® Cu(s). 5. Which of the following statements about the voltaic cell shown...
Please explain why Which of the following statements is true for the voltaic cell using the...
Please explain why
Which of the following statements is true for the voltaic cell using the reaction: Cu(s) + 2Ag+(aq) + 2Ag(s) + Cu2+(aq) Electrons spontaneously flow from the Cu electrode to the Ag electrode. Electrons spontaneously flow from the Ag electrode to the Cu electrode. O Cations migrate from the salt bridge into the Cu electrode compartment. O none of these
Part A Consider a voltaic cell that is set up as follows: Anode contains an Zn(s) electrode and 1M Zn2+(aq) Cathode cont...
Part A Consider a voltaic cell that is set up as follows: Anode contains an Zn(s) electrode and 1M Zn2+(aq) Cathode contains a Pt(s) electrode and 1M MnO4–(aq),Mn2+(aq), and H+(aq) Which of the following statements match the cathode? Select all that apply. Group of answer choices The electrode increases in mass Oxidation occurs at this half-cell Electrons enter the half-cell The electrode is inactive Cations from the salt-bridge move to this half-cell The electrode is negative Part B Which of...
Folder# Grade 1. In the voltaic cell shown below, the electrons flow from Zn(s)|Zn²+ (aq)|| Cu"...
Folder# Grade 1. In the voltaic cell shown below, the electrons flow from Zn(s)|Zn²+ (aq)|| Cu" (aq)|Cu(s) Cu(s) (a) Cu(s) ® Zn(s) (b) Zn(s) (c) Zn(s) ® cu (d) Cut ® Zn(s) 2. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq) Cu(s) (a) Oxidation takes place at the cathode and reduction takes place at the anode. (b) Oxidation takes place at both the cathode and the anode. (c) Reduction takes place...
1a) In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as...
1a) In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Zn(s)|Zn2+(aq)||H+(aq)|H2(g)|Pt(s) Select one or more: Zn/Zn2+ is the anode Eºcell is positive H+/H2 is the cathode Zn/Zn2+ is the cathode H+/H2 is the anode Eºcell is negative
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr Cr3+ half cell and the cathode is a SnSn2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: + + In the external...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)
3. The following redox couple was used in the construction of a voltaic cell. (All ions are in aqueous solution and you ned to decide which haif resetion wil e in he cahode side and wh the cathode side and which in the anode side.) For the cell: . Make a sketch of the cell labeling anode, cathode, salt bridge (using KNOs), direction of electron flow, oxidation half ell, reduction half cell, charge of the anode, charge of the cathode,...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
20) 20) Which of the following statements concerning a voltaic cell is FALSE A) At the anode a substance will lose electrons. B) A voltaic cell uses an oxidation-reduction reaction to produce electrical energy. C) The oxidation half reaction occurs at the cathode. D) The cell consists of two half cells. E) The anode and the cathode are separated by a salt bridge. - 21) The fluoride rinse in dental offices usually contains sodium fluoride, Sodium fluoride 2 1 can...
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq)|Cu(s) (a) The oxidation half-reaction is clearly Zn(s) ® Zn** (aq) + 2 e. (b) The oxidation half-reaction is clearly Zn() Zn" (aq) +le. (C) The oxidation half-reaction could not be anything other than Cu(s) ® Cu (aq) +2 e. (d) It is obvious that the oxidation half-reaction is Zn(s) ® Cu(s). 5. Which of the following statements about the voltaic cell shown...
Please explain why
Which of the following statements is true for the voltaic cell using the reaction: Cu(s) + 2Ag+(aq) + 2Ag(s) + Cu2+(aq) Electrons spontaneously flow from the Cu electrode to the Ag electrode. Electrons spontaneously flow from the Ag electrode to the Cu electrode. O Cations migrate from the salt bridge into the Cu electrode compartment. O none of these
Folder# Grade 1. In the voltaic cell shown below, the electrons flow from Zn(s)|Zn²+ (aq)|| Cu" (aq)|Cu(s) Cu(s) (a) Cu(s) ® Zn(s) (b) Zn(s) (c) Zn(s) ® cu (d) Cut ® Zn(s) 2. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq) Cu(s) (a) Oxidation takes place at the cathode and reduction takes place at the anode. (b) Oxidation takes place at both the cathode and the anode. (c) Reduction takes place...
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