Consider an electrolytic cell with a steady voltage of 4.6 V which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below.2A1,0 3(1)+ 3CO(s)+3C(s)- 4AI2(g)What will be the magnitude of the electrical energy in kWh needed to produce 216 g of Al(s)?Show your answers in two decimal places. Do NOT include units in your final answer.

Answered: Image /qna-images/answer/8f17455f-3d6c-4252-8cea-6c3f71494a9f.jpg

Consider an electrolytic cell with a steady voltage of 4.6 V which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 3(1) + 3C (s) - 4AI + 3CO (8) 2(g) What will be the magnitude of the electrical energy in kWh needed to produce 216 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.

Consider an electrolytic cell with a steady voltage of 4.6 V which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 3(1) + 3C (s) - 4AI + 3CO (8) 2(g) What will be the magnitude of the electrical energy in kWh needed to produce 216 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.

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...

See similar textbooks

Similar questions

A certain metal M forms a soluble sulfate salt M2(SO4)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of M₂(SO4)3 the right half cell with a 15.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left ☐ x10 O right Π
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
A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M₂SO4 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. V left right x10 X T
A certain metal M forms a soluble nitrate salt M (NO3)₂. Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M 2 solution of M (NO3), and the right half cell with a 50.0 mM solution of the same substance. Electrodes made of M are dipped into 2 both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 left right x10 X
In an car battery recharging occurs when the car is running by supplying a current to the battery. The reaction that occurs at the cathode in this electrolytic process is Pb2+ + 2e- --> Pb (s) If the car supplies a current of 1.50A to the battery, how long will it take in minutes to have 25.0 g of Pb(s) collected at the cathode? Hint: Start with 25.0 g Pb (1A = 1C/sec) (F= 96500 C/mole e-) (Pb =207.2g/mol) Answer has 3 sig figs
Qd 125.
2 A certain metal M forms a soluble nitrate salt M(NO3)₂. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.00 M solution of M(NO3), and the right half cell with a 100. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. left x10 Which electrode will be positive? right X ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
4
A certain metal M forms a soluble nitrate salt M (NO₂), Suppose the left half cell of a galvanic cell apparatus is filled with a 40.0 mM solution of M(NO), and the right half cell with a 4.00 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O left O right 0 0.2 X Glo Ar
A certain metal M forms a soluble nitrate salt M(NO3). Suppose the left half cell of a galvanic cell apparatus is filled with a 4.00 M solution of M(NO3), and the right half cell with a 200. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left ☐ x10 right
Handwriting not allow please
Consider an electrolytic cell with a steady current of 169 amperes which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 31) + 3C (s) -4AI +3CO (s) 2(g) What is the time, in hours, needed to produce 218 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.