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...
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.
(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.
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.
(7. Consider the reaction as follows: Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 NaCl(aq) A 1.00-mol sample of sodium sulfate was placed into the barium chloride aqueous solution to make solid barium sulfate. (a) How many gram of sodium sulfate was placed into the reaction solution? (b) What is the maximum mass of NaCl formed? (c) If 78.9 g of NaCl was obtained, what was the percent yield of NaCl? 3. How many liters of 0.186 M of NaOH (aq)...
Aqueous hydrochloric acid (HCl) reacts with solid hydroxide (NaOH) to produce aqueous sodium chloride (NaCl) and liquid water H2O. If 1.23 g of sodium chloride is produced from the reaction of 2.2 g of hydrochloric acid and 4.6 g of sodium hydroxide, calculate the percent yield of sodium chloride. Round your answer to 2 significant digits.
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: 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...
The gas OF2 can be produced from the electrolysis of an aqueous solution of KF, as shown in the equation below. OF2(g) + 2 H+(aq) + 4 e- → H2O(l) + 2 F-(aq) E° = +2.15 V Using the given standard reduction potential, calculate the amount of OF2 that is produced, and the electrode at which the OF2 is produced, upon the passage of 0.120 faradays through an aqueous KF solution. The gas OF2 can be produced from the electrolysis...
Solution Stoichiometry Hydrochloric acid (HCl) reacts with sodium carbonate (Na2CO3), forming sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2). This equation is balanced as written: 2HCl(aq)+Na2CO3(aq)→2NaCl(aq)+H2O(l)+CO2(g) a) What volume of 2.75 M HCl in liters is needed to react completely (with nothing left over) with 0.750 L of 0.300 M Na2CO3? b) A 565-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 10.1 g CO2. What was the concentration of the HCl solution? How do I...