d) During the electrolysis of
brine, gradually chloride ions are converted into chlorine gas,
H+ ions from water produce hydrogen gas. -OH-
are also formed from water and they combine with Na+
ions in aqueous phase.
Both the H2 gas and Cl2 gas may combine and the reaction is explosive. So to avoid this reaction, the cathode must be surrounded by a porous diaphragm made of asbestos.
The diaphragm is chosen in such a way that it allows the flow of Na+ ions from anode. Then the Na+ ions combine with OH- ions formed in cathode cell.
The electrolyte brine gradually converts into sodium hydroxide solution.
Name: Electrochemistry and Equivalent Mass Figure 4: Electrolysis of NaCl(a) "brine" solution. 4. Refer to...
An important industrial reaction is the electrolysis of brine to form chlorine and sodium hydroxide. At one of the electrodes, chloride ions are oxidized to form chlorine. The overall reaction is: 2NaCl + 2H2O à 2NaOH +Cl2 + H2 A. Determine the electrode reactions (i.e., oxidation and reduction reactions). B. Identify the anode and cathode as well as their signs (i.e., positive and negative electrode). C. Determine the direction of current flow. D. Calculate the standard cell potential.
Need help with question 1. A-F
Name: ELECTROCHEMISTRY WORKSHEET 1. Answer the questions below regarding the voltaic cell drawn. NO Cathode NO, BI Anode NO3- NO3 NO, NO, a. Write both half reactions: Cathode Half Reaction: Anode Half Reaction: b. In which direction will the electrons flow? c. Which electrode will be positively charged? d. In which direction will the NO3 ions flow in the salt bridge? e. Which electrode decreases in mass during the reaction? f. Write the shorthand...
An industrial process referred to as the Downs cell converts molten sodium chloride into its constituent elements through electrolysis. The cell consists of a mixture (40%) of NaCl in CaCl2 (60%) at 600°C. Calcium ions do not participate in the reaction. The graphite anode is encircled by a steel cathode. Sodium floats over the denser electrolyte and is conveyed to a reservoir while chlorine gas escapes through a vertical pipe.[10]a. Identify the oxidizing and the reducing agent (1)b. Draw a...
Experiment 9 Part C-Electrolysis of Salt Solutions 10. Obtain and thoroughly rinse a U-shaped glass tube (U-tube) and fill it to within an inch or so of the rim with the 2% NaCl solution. 11. Add one drop of phenolphthalein to each arm of the U-tube. Clamp the U-tube to a ring stand (Figure 9-2). 12. Obtain two graphite electrodes and rinse the electrodes thoroughly. Obtain two connector wires with alligator clamps on both ends. With one of the clamps...
Electrolysis of sea water (NaCl(aq)) produces Cl2(g) at the anode, and H2(g) and NaOH(aq) at the cathode. For such a cell operating under standard conditions, the minimum voltage (volts) required to drive the reaction is A. 3.02 B. 0.83 C. 1.36 D. 1.66 E. 2.1 9
NAME: General Chemistry II Electrochemistry Quiz 1) Consider the cell described by: Cu Cu2+ (1.00 M) || Zn2+(1.00M) | Zn a) Draw this cell, labeling everything including the cathode, anode and salt bridge and any ions in solution. Show the flow of electrons in the circuit. b) Write out the reduction and oxidation half reactions for this cell. OVER → 2) Balance the following redox equations using the half-reaction method. Show all steps. a) ClO3 + + CH-1 → Cl2...
What is the effect on the emf of the cell shown in Figure 20.9, which has the overall reaction Zn(s)+2H+(aq)Zn(s) +2 H+(aq) −→−Zn2+(aq)+H2(g),→ Zn2+(aq) + H2(g), for each of the following changes? The pressure of the H2H2 gas is increased in the cathode half-cell. Zinc nitrate is added to the anode half-cell. Sodium hydroxide is added to the cathode half-cell, decreasing [H+].[H+]. The surface area of the anode is doubled. Can someone please explain why b is emf decreases? Why...
Sodium hydroxide can be produced by electrolysis of NaCl solution 2NaCl(aq) + 2 H2O(l) à 2 NaOH(aq) + H2(g) + Cl2(g) A 100 g of 20 % aqueous solution of NaClwas used and conversion of NaCl is 90 %. Neglecting solubility of H2 and Cl2 in water, calculate % NaOH in the aqueous product. Use molecular balance method.
Sodium hydroxide can be produced by electrolysis of NaCl solution 2NaCl(aq) + 2 H2O(l) à 2 NaOH(aq) + H2(g) + Cl2(g) A 100 g of 20 % aqueous solution of NaClwas used and conversion of NaCl is 90 %. Neglecting solubility of H2 and Cl2 in water, calculate % NaOH in the aqueous product. use molecular balance method
Plz Help Me
Part 4: Electrolysis Check out a conductivity kit from the stockroom window (includes well-plate and well-charged 9V battery). You will make observations on three solutions. Fill the oblong well with distilled water for rinsing the electrodes. First well: Fill the well 2/3 full with 0.1 M Na SO, +one drop of phenolphthalcin. Place the electrodes into the solution. Look carefully around cach cloctrode. You may see the appearance of color or the disappearance of color, as well...