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
3.02
0.83
C. 1.36
1.66
2.1
9
Electrolysis of sea water (NaCl(aq)) produces Cl2(g) at the anode, and H2(g) and NaOH(aq) at the...
(a) In the electrolysis of aqueous NaCl, how many liters of H2(g) (at STP) are generated by a current of 85.4 A for a period of 69.2 min? The unbalanced chemical reaction representing this electrolysis is shown below. NaCl(aq) + H2O(l) --> Cl2(g) + H2(g) + NaOH(aq) _____ liters of H2(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the solution in this process? _____ moles of NaOH(aq) are formed.
(a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 80.1 A for a period of 64.6 min? The unbalanced chemical reaction representing this electrolysis is shown below. NaCl(aq) + H2O(l) → C12(9) + H2(g) + NaOH(aq) liters of Cl2(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the solution in this process? moles of NaOH(aq) are formed.
What product forms at the anode in the aqueous electrolysis of MnCl2? Cl2(g) Mn(s) H2(g) and OH -(aq) O2(g) and H+(aq)
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
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
Name: Electrochemistry and Equivalent Mass Figure 4: Electrolysis of NaCl(a) "brine" solution. 4. Refer to figure 4, an illustration of the electrolysis of a NaCl(aq) solution, called a brine". This method is used to manufacture chlorine gas and sodium hydroxide. Chlorine is widely used to purify water, as a disinfectant, and in the making of important compounds such as chloroform, a compound used in the production of Teflon. Chloride ions are oxidized in the anode half-cell and water is reduced...
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.136 M), mixed with its conjugate base, A-(0.142 M). The measured cell voltage is E°cell = 0.196 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = _______ Ka = _______
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.160 M), mixed with its conjugate base, A-(0.120 M). The measured cell voltage is E°cell = 0.228 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = Ka =
A chemical plant uses electrical energy to decompose aqueous solutions of NaCl to give Cl2, H2, and NaOH: 2NaCl(aq)+2H2O(l)→2NaOH(aq)+H2(g)+Cl2(g) 1. If the plant produces 1.6×106 kg (1600 metric tons) of Cl2 daily, estimate the quantities of H2 produced. 2. If the plant produces 1.6×106 kg (1600 metric tons) of Cl2 daily, estimate the quantities of NaOH produced.