Industrial Processes for Ammonia and Nitric Acid
Chemistry ⇒ Industrial Chemistry
Industrial Processes for Ammonia and Nitric Acid starts at 11 and continues till grade 12.
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Calculate the mass of ammonia produced from 28 g of nitrogen gas, assuming excess hydrogen and 100% yield. (Molar mass N2 = 28 g/mol, NH3 = 17 g/mol)
Calculate the number of moles of ammonia produced when 3 moles of hydrogen react completely with excess nitrogen according to the Haber-Bosch equation.
Calculate the volume of ammonia gas produced at STP from 2.0 moles of nitrogen gas, assuming excess hydrogen. (Molar volume at STP = 22.4 L/mol)
Describe one method by which hydrogen is industrially obtained for the Haber-Bosch process.
Describe the environmental impact of ammonia production on the atmosphere.
Describe the importance of the Haber-Bosch process in global agriculture.
Describe the role of water in the Ostwald process.
Explain why a compromise temperature is used in the Haber-Bosch process.
Explain why ammonia is liquefied during its industrial production.
Explain why the Haber-Bosch process is considered an example of chemical equilibrium.
Explain why the Ostwald process is considered a catalytic process.
Explain why the Ostwald process is important for the explosives industry.
In the context of the Ostwald process, what is the main environmental concern associated with nitrogen oxides?
State one reason why high pressure is used in the Haber-Bosch process.
State the chemical formula for nitric acid.
State the role of the iron catalyst in the Haber-Bosch process.
The overall reaction for the Ostwald process is: 4NH3 + 5O2 → 4NO + 6H2O. How many moles of NO are produced from 8 moles of NH3?
What is the balanced chemical equation for the synthesis of ammonia in the Haber-Bosch process?
