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. (N = 14, H = 1)
Calculate the number of moles of ammonia produced when 3 moles of nitrogen react completely with excess hydrogen in the Haber process.
Describe one way in which the efficiency of the Haber process can be improved.
Describe the importance of recycling unreacted gases in the Haber process.
Describe the role of the iron catalyst in the Haber process.
Explain why ammonia is liquefied in the Haber process after synthesis.
Explain why high pressure is used in the Haber process.
Explain why the Haber process is important for global food production.
Explain why the Ostwald process is considered a catalytic process.
Explain why the Ostwald process is considered an example of green chemistry.
In the context of the Haber process, what is meant by 'dynamic equilibrium'?
In the Haber process, what is the effect of increasing the temperature on the equilibrium yield of ammonia?
In the Ostwald process, ammonia is oxidized to produce which acid?
In the Ostwald process, nitrogen monoxide (NO) is further oxidized to form which compound?
In the Ostwald process, what is the function of cooling the reaction mixture after the oxidation of ammonia?
State one environmental impact of the large-scale production of ammonia.
State one reason why a moderate temperature is used in the Haber process instead of a very high temperature.
State the main reason why the Haber process is not carried out at very low temperatures.
Write the balanced chemical equation for the first step of the Ostwald process.
Write the balanced chemical equation for the reaction of nitrogen dioxide with water in the Ostwald process.
