Use the following information to answer the next question. Hydrogen-oxygen fuel cells have been used for years in spacecraft and more recently in small-scale power plants to generate electricity. Now, some governments and companies are working together to perfect this type of fuel cell for automobile use, and experiments are currently being conducted with operational prototypes. A diagram of a hydrogen-oxygen fuel cell is shown below. 4H₂O Porous carbon electrodes containing catalysts H₂ OH H₂O O In the diagram above, the product of the reaction, the electrolyte, the anode, and the cathode are labelled, if written as a singular four digit number it would be

Use the following information to answer the next question. Hydrogen-oxygen fuel cells have been used for years in spacecraft and more recently in small-scale power plants to generate electricity. Now, some governments and companies are working together to perfect this type of fuel cell for automobile use, and experiments are currently being conducted with operational prototypes. A diagram of a hydrogen-oxygen fuel cell is shown below. 4H₂O Porous carbon electrodes containing catalysts H₂ OH H₂O O In the diagram above, the product of the reaction, the electrolyte, the anode, and the cathode are labelled, if written as a singular four digit number it would be

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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Many underground pipes are protected from corrosion by connecting them by a conducting wire to a block of magnesium metal buried close to the pipe. The magnesium protects the iron by acting as a sacrificial anode. Another metal which could also act as the sacrificial anode would be zinc mercury copper O nickel silver
4. In the electrolysis of a sodium chloride solution, what volume of Cl2 (g) is produced in the same time it takes to produce 6.0 L of H2(g), both volumes measured at 0 °C and 1.0 atm?
The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction is given below. 2 H2O(l) + 2 e− → H2(g) + 2 OH− (aq) Hydroxide ion reacts with lactic acid as soon as it is produced. The endpoint of the reaction is detected with an acid-base indicator. It required 104 s for a current of 13.1 mA to reach the endpoint. How many grams of lactic acid (a monoprotic acid) were present in the sample?
The process of decomposition of an electrolyte by passing electric current through its solution is called as Electrochemical cell .a O Electrolysis .b O Electrolyte .c O Electrode .d O
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
7. Fig. 7.1 shows a simplified diagram of the electrolysis of sodium chloride solution, used to produce chlorine in industry. concentrated sodium chloride solution anode cathode gas 111 chlorine gas permeable membrane hydrogen Fig. 7.1 The balanced equation for the overall chemical change that occurs in the process shown in Fig. 7.1 is 2NaCl + 2H₂O → 2NaOH + Cl₂ + H₂ a. Show that the relative formula mass of sodium chloride is 58.5 sodium hydroxide solution b. Calculate the number of moles in 234g of sodium chloride. Show your working. Number of moles= Volume= c. Calculate the volume of chlorine molecules produced at room temperature and pressure, when 234g of sodium chloride are electrolysed. (1 mole of chlorine molecules has a volume of 24 dm³ at room temperature and pressure). Show your working
You are a bioengineer designing a new type of pacemaker. Which type of Galvanic cell would be best for you to use in this new device?
A certain metal M forms a soluble nitrate salt M(NO3)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M(NO3)3 and the right half cell with a 10.0 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 20.0 °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 0 ○ left ☐ x10 O right ×
A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V).The button form of this cell is used in watches, hearing aids, and other electronic devices.The half-reactions are:Zn(s) + 2OH- (aq) → Zn(OH)2(s) + 2eAg2O(s) + H2O(l) + 2e- → 2Ag(s) + 2OH(aq)(a) Identify the anode and the cathode reactions.(b) What’s the overall reaction in this galvanic cell?
A certain metal M forms a soluble nitrate salt M(NO3)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M(NO3)3 and the right half cell with a 30.0 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 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. ☐ left ☐ x10 right ☑
Which statement about electrolytic cells is false? Electrolytic cells convert electrical energy into chemical energy. O The redox reaction is non-spontaneous. The anode and cathode are placed in the same container with the aqueous electrolyte. O The anode is negative and the cathode is positive. O The external battery supplies the electrons.