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 chlorine gas H permeable membrane cathode Fig. 7.1 hydrogen gas 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

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 chlorine gas H permeable membrane cathode Fig. 7.1 hydrogen gas 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

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

Chapter20: The Representative Elements

Section: Chapter Questions

Problem 18E

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When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?
Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.
Oxygen is not normally found in positive oxidation states, but when it is combined with fluorine in the compound oxygen difluoride, oxygen is in a +2 oxidation state. Oxygen difluoride is a strong oxidizing agent that oxidizes water to produce O2 and HF. OF2(g) + H2O(g) → 2 HF(g) + O2(g) The standard formation enthalpy of oxygen difluoride is 24.5 kJ/mol. Using this information and data from Appendix J, calculate the standard reaction enthalpy for the reaction of oxygen difluoride with water. Table 4.2 Selected Standard Formation Enthalpies, ΔfH°, at 25°C
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Zinc is produced by electrolytic refining. The electrolytic process, which is similar to that for copper, can be represented by the two half-reactions Zn(impure,s)Zn2++2eZn2++2eZn(pure,s) For this process, a voltage of 3.0 V is used. How many kilowatt hours are needed to produce one metric ton of pure zinc?
• write and balance half-reactions for simple redox processes.
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4 ions by periodate ion (IO4) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate and G at 25C for each reaction.
Electrochemical Cells II Consider this cell running under standard conditions: Ni(s)Ni2(aq)Cu+(aq)Cu(s) a Is this cell a voltaic or an electrolytic cell? How do you know? b Does current flow in this cell spontaneously? c What is the maximum cell potential for this cell? d Say the cell is connected to a voltmeter. Describe what you might see for an initial voltage and what voltage changes, if any, you would observe as time went by. e What is the free energy of this cell when it is first constructed? f Does the free energy of the cell change over time as the cell runs? If so, how does it change?
One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?

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