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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A plant absorbs 10,000 moles of SO3 in concentrated H2SO4. How many moles of oleum are formed?
A plant produces 490 kg of H2SO4 per hour. How many moles of H2SO4 is this? (Molar mass = 98 g/mol)
Calculate the mass of SO2 required to produce 98 g of H2SO4 (Assume 100% yield). (Molar masses: SO2 = 64 g/mol, H2SO4 = 98 g/mol)
Calculate the volume of oxygen (at STP) required to completely oxidize 128 g of SO2 to SO3. (Molar mass SO2 = 64 g/mol, 1 mol gas at STP = 22.4 L)
Describe one method used to minimize the release of SO2 into the atmosphere during sulfuric acid production.
Describe the environmental impact of sulfuric acid mist if released into the atmosphere.
Describe the role of absorption towers in the Contact process.
Describe the three main stages of the Contact process for manufacturing sulfuric acid.
Explain the importance of using a catalyst in the Contact process.
Explain the significance of the Contact process in the global chemical industry.
Explain why a moderate temperature is used in the catalytic oxidation step of the Contact process.
Explain why the absorption of SO3 is not done directly in water during the Contact process.
Explain why the Contact process is preferred over the Lead Chamber process for modern sulfuric acid production.
In the Contact process, why is excess oxygen used during the oxidation of SO2?
State the role of vanadium(V) oxide in the Contact process.
What is the balanced chemical equation for the catalytic oxidation of sulfur dioxide in the Contact process?
