Telephone Number: 7738-17 Email: tpchrdnova@gmail.com NAME: GRADE & SECTION: SUBJECT TEACHER: ACTIVITY SHEET in CHEMISTRY 2 WEEK 5-6 1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of MnO-4MnO4- in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn2+Sn2+ in dilute sulfuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2MnO-4(aq)+5Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+(aq)+8H2O(1)2MnO4-(aq)+5 Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+(aq)+8H2O(1) For this galvanic cell, 1. write the half-reaction that occurs at each electrode. Sour 2. indicate which electrode is the cathode and which is the anode. 3. indicate which electrode is positive and which is negative. ng, document you via e-mail cathe tht reflects fre allel to the in flecto ncor vith ig n

Telephone Number: 7738-17 Email: tpchrdnova@gmail.com NAME: GRADE & SECTION: SUBJECT TEACHER: ACTIVITY SHEET in CHEMISTRY 2 WEEK 5-6 1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of MnO-4MnO4- in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn2+Sn2+ in dilute sulfuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2MnO-4(aq)+5Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+(aq)+8H2O(1)2MnO4-(aq)+5 Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+(aq)+8H2O(1) For this galvanic cell, 1. write the half-reaction that occurs at each electrode. Sour 2. indicate which electrode is the cathode and which is the anode. 3. indicate which electrode is positive and which is negative. ng, document you via e-mail cathe tht reflects fre allel to the in flecto ncor vith ig n

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Suppose the galvanic cell sketched below is powered by the following reaction: Mg(s)+CuCl,(aq) MgCl,(aq)+Cu(s) e- E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cellI. O- Write a balanced equation for the half-reaction that happens at the anode of this cell. 0,0. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
consider these two entries from a ficitional table of standard reduction potentials. (see image) what is the standard potential of a galvanic (voltaic) cell? give answer to 3 sig figs inputting only the numeric value, assuming a measurement of V
Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
A standard galvanic cell is constructed in which a Co2+ | Co half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The cathode reaction is Co2+ + 2e -> Co. Co is oxidized at the cathode. The anode compartment could be Fe³+|Fe²+. As the cell runs, anions will migrate from the Co²+ | Co compartment to the other compartment. In the external circuit, electrons flow from the Co²+ | Co compartment to the other compartment.
Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 中 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? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 G
Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell V
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O ELECTROCHEMISTRY Designing a galvanic cell from tw... A chemist designs a galvanic cell that uses these two half-reactions: standard reduction half-reaction 2H₂O(1)+2e Write a balanced equation for the half-reaction that happens at the anode. Ered= Br₂(1)+2e Ered = +1.065 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. 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? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. 0 0 0 O Yes O No H₂(g) + 2OH(aq) 2 Br (aq) V potential = -0.83 V - 3 ⠀ ローロ X 2 5 x10 S
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2. In the electrolysis of an aqueous Zn(NO3)2 solution, what reactions occur at the anode and at the cathode, assuming standard conditions? O, + 4H + 4e → 2H;O 6° = 1.23 V 2H,0 + 2e → H2 + 20H E° = -0.83V Zn2 + 2e → Zn ɛ° = -0.76 V NO, + 4H + 3e' → NO + 2H20 E° = 0,96 V ANODE: CATHODE:
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A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…