Industrial Processes for Sodium Hydroxide and Chlorine
Chemistry ⇒ Industrial Chemistry
Industrial Processes for Sodium Hydroxide and Chlorine starts at 11 and continues till grade 12.
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See sample questions for grade 11
A plant produces 1000 kg of NaOH per day. How many moles of NaOH does it produce per day? (Na = 23, O = 16, H = 1)
Calculate the mass of chlorine gas produced when 2 moles of NaCl are electrolyzed completely.
Describe one advantage of the membrane cell process over the mercury cell process.
Describe the environmental impact of the diaphragm cell process.
Describe the main difference between the mercury cell and membrane cell processes.
Explain why brine is purified before use in the chlor-alkali process.
Explain why it is important to keep chlorine and sodium hydroxide separated during the industrial process.
Explain why the production of sodium hydroxide and chlorine is considered an example of a redox reaction.
Explain why the purity of sodium hydroxide is higher in the membrane cell process than in the diaphragm cell process.
In the diaphragm cell process, what is the main purpose of the diaphragm?
Name one major use of sodium hydroxide produced in the chlor-alkali industry.
Name the three main industrial processes used for the production of sodium hydroxide and chlorine.
State one major environmental concern associated with the mercury cell process.
State one reason why the membrane cell process is preferred over the diaphragm cell process.
State the cathode reaction in the electrolysis of brine.
State the main reason for using a direct current (DC) in the electrolysis of brine.
What is the role of hydrogen gas produced in the chlor-alkali process?
Which electrode is chlorine gas produced at during the electrolysis of brine?
Write the balanced chemical equation for the electrolysis of brine to produce sodium hydroxide and chlorine.
