Industrial Processes for Sulfuric Acid
Chemistry ⇒ Industrial Chemistry
Industrial Processes for Sulfuric Acid starts at 11 and continues till grade 12.
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Calculate the mass of SO3 produced from 64 g of SO2 (Molar mass: SO2 = 64 g/mol, SO3 = 80 g/mol) in the reaction: 2 SO2 + O2 → 2 SO3.
Calculate the number of moles of SO3 produced from 4 moles of SO2 in the reaction: 2 SO2 + O2 → 2 SO3.
Describe one environmental concern associated with the industrial production of sulfuric acid.
Describe the environmental impact of releasing SO2 into the atmosphere from sulfuric acid plants.
Describe the purpose of the absorption tower in the Contact process.
Explain why high pressure is not commonly used in the Contact process, even though it favors the formation of SO3.
Explain why impurities such as dust and arsenic compounds must be removed from SO2 before it enters the catalytic converter in the Contact process.
Explain why the Contact process is considered an example of a reversible reaction.
Explain why the Contact process is important for the global economy.
In the Contact process, why is air used instead of pure oxygen for the oxidation of SO2?
In the Contact process, why is the temperature kept around 450°C for the catalytic oxidation of SO2?
Name the intermediate compound formed when SO3 is absorbed in concentrated sulfuric acid.
State one reason why direct absorption of SO3 in water is not used in the Contact process.
State the main reason why the Contact process replaced the Lead Chamber process for sulfuric acid production.
What is the chemical formula of oleum?
What is the main advantage of using a catalyst in the Contact process?
What is the main industrial use of oleum?
What is the role of the catalyst in the Contact process?
Write the balanced chemical equation for the oxidation of sulfur dioxide to sulfur trioxide in the Contact process.
