Hydrazine, N, B4, has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. Thereactions are as follows.N,H4 (ag) + 40H (ag) N(9) + 4 H,0(1) + 4 e02 (9) + 2 H2O(1) + 4 e 4 OH (ag)(a) Which reaction occurs at the anode and which at the cathode?N,H4 (ag) + 4 0H (ag) N2(9) + 4 H,0(1) + 4 e02 (9) + 2 H,0(1) + 4 e→ 4 OH (aq)(b) What is the net cell reaction? (Include states of matter in your answer. Leave any unneeded answerblanks empty.)(c) If the cell is to produce 0.54 A of current for 48.0 h, what mass in grams of hydrazine must bepresent?(d) What mass in grams of O2 must be available to react with the mass of N2 H. determined in part (c)?

a) Since in given reaction, O2 is reduced whereas hydrazine(N2H4) is oxidized because of electrons…

Answered: Hydrazine, N, H, has been proposed as…

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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Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr3+ (aq) and a cathode where Cr3+ (aq) is reduced to Cr2+ (aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
+ 2+ MnO 4(aq) +8 H (aq) +5e → Mn(aq) + 4H₂O(1) 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. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? 3+ If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to significant digits. Fe half-reaction 0 (aq) + e Yes No V 2+ Fe (aq) standard reduction potential red 'red = +1.51 V = +0.771 V ローロ x 90 x10 S
Please explain and give the correct answers.
For the following reaction, predict the measured cell potential (Ecel) if the pressure of O2 is 1.59 atm, the concentration of H* is 9.67 x 103 M and the bromide ion concentration is 1.31 M. 0, (g) + 4H* (ag) + 4Br (aq) → 2H,O() + 2Br, () Half reactions: 2Br, () + 4e→ 4Br (aq) E° = +1.077 V 0,(g) + 4H* (aq) + 4e→ 2H,0(1) E° = +1.229 V
How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water with a current of 4.52 A for a period of 2.77 minutes? The cathode reaction is 2H₂O + 2e → H₂ + 2OH- mol OH = =
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) + 3 Ca(s) → 2Cr(s) + 3Ca²+ (aq) Suppose the cell is prepared with 6.35 M Cr³+ in one half-cell and 0.492 M Ca2+ in the other half. Calculate the cell voltage under these conditions. Cr3+ (aq) + 3e → Cr(s) Ered = -0.744 V Ca2+ (aq) + 2e → Ca(s) Ered = -2.868 V The standard cell potential (E°) for this galvanic cell is [Select] V. There are [ Select] + moles of electrons transferred during to operate this galvanic cell. Under these conditions, the reaction quotient is [Select] and the cell volatage is [Select] V. In order to increase the cell voltage for this cell, [Select ]
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: MnO₂ (s) + 4H* (aq) + 2Cr²+ (aq) → Mn²+ (aq) + 2H₂O (1) + 2Cr³+ (aq) 2+ 2+ 3+ Suppose the cell is prepared with 3.73 MH* and 1.42 M Cr²+ in one half-cell and 4.21 M Mn²+ and 3.05 M Cr³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 1 x10 X μ 00 Ś
Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode
Write the anodic and cathodic half-reactions that take place when a piece of galvanized steel is corroded in an acidic medium (pH = 4.5).
A student wanted to measure the concentration of cobalt(II) ion in an aqueous solution. For the cathode half-reaction, she used a silver electrode with a 0.51 M solution of AgNO3. For the anode half-reaction, she used a cobalt electrode dipped into the aqueous solution. If the cell gave a potential of 1.043 V at 25 °C, what was the concentration of Co2+ in the solution? Half-reaction E° (V) Ag*(aq) + e- Ag(s) +0.7996 Co2+(aq) + 2 e- -0.28 Co(s) Your Answer: Answer units
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) +5Co²+ (aq) 2+ Suppose the cell is prepared with 5.23 M IO3 and 2.31 M H in one half-cell and 6.84 M Co in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+ (aq) + 3Ca (s) → 2Cr (s) + 3 Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 2.68 M Cr in one half-cell and 7.85 M Ca in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロ・ロ × μ 0|0 Ś

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