1. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas = P bar - VP mm Hg = atm water V hydrogen gas mL T = K n hydrogen gas moles

1. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas = P bar - VP mm Hg = atm water V hydrogen gas mL T = K n hydrogen gas moles

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

Please don't provide handwritten solution
Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to measure the amount of electricity passing through a circuit. In this meter, a small, fixed fraction of the total current supplied to a household was passed through an electrolytic cell, plating out zinc at the cathode. Each month the cathode could then be removed and weighed to determine the amount of electricity used. If 0.25% of a household’s electricity passed through such a coulometer and the cathodeincreased in mass by 1.83 g in a month, how many coulombs of electricity were used during that month?
A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 225. mM solution of MNO3 and the right half cell with a 4.50 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 35.0 °C. x10 Which electrode will be positive? left right X Ś ? 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.
The silver zinc battery is used in hearing aids. Explain the fundamental redox reactions that occur in this battery and calculate the theoretical cell potential for this system.
In an electrochemical cell, a metal anode lost 0.286 g while a total volume of 0.04854 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 763.5 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the molar mass of the metal?
You make a voltaic cell with copper and aluminum. If the cell potential is measured to be +2.50 V at room temperature, then what is the reaction quotient?
6) Calculate the potential of a cell, Eºcell, made with a standard bromine electrode as the anode and a standard chlorine electrode as the cathode. Write the shorthand cell notation.
231. Subject :- Chemistry
. A factory wants to produce 1.0 x 10° kg Barium from the electrolysis of molten barium chloride. What current must be applied for 4.0 h to accomplish this?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGO. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell n A U calculated quantities (Check the box next to any that are wrong.) AGⓇ -117. kJ/mol - 129. kJ/mol 112. kJ/mol K 3.18 × 10 2.51 X 10 4.18 × 10 21 - 23 19 0 E 1.21 V - 1.34 V 1.16 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E". His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V