Use a copy of the Periodic Table where you need one.
Which statement about the iron catalyst in the Haber process is correct?
Source: Learners' Alley, Ammonia slides
Which change increases the yield of ammonia in the Haber process?
Source: Learners' Alley, Ammonia slides
Answer these questions about the Haber process.
Source: Learners' Alley, Ammonia slides
Which reaction is irreversible?
Source: Learners' Alley, Ammonia slides
Solid ammonium chloride is heated in a test tube. A piece of damp red litmus paper is held at the mouth of the tube.
Source: Learners' Alley, Ammonia slides
In the Haber process, nitrogen and hydrogen react to form ammonia. What is the source of hydrogen?
Source: 2024 AMKSS Prelim P1 Q15
Which statement about the Haber process is not correct?
Source: 2024 Dunman Prelim P1 Q25
Which statement about the manufacture of ammonia in the Haber process is incorrect?
Source: 2024 CHIJ Prelim P1 Q17
Which of the following can increase the yield of ammonia in the Haber process?
Source: 2024 AMKSS Prelim P1 Q16
Ammonia gas is produced using the Haber process. Which statement best explains why a higher temperature of 450 °C is used, although a lower temperature of 250 °C produces a higher yield of ammonia?
Source: Broadrick Prelim P1 Q23
Which statement about the Haber process is correct?
Source: 2024 SJI Prelim P1 Q17
Ammonia gas can be made industrially by reacting nitrogen with hydrogen in the Haber process. The conditions are 450 °C and 250 atm, with finely divided iron as the catalyst. The reaction is reversible.
Source: 2023 XMS Sec 3 WA3 Q7(b)
The Haber process uses iron as a catalyst and involves a reversible reaction.
Source: 2024 Jurongville Prelim P2 Q7(b)
The Haber process is used to manufacture ammonia in the chemical industry.
Source: 2022 SJI Prelim P2 A3(c)
BIt speeds up the reaction.[1]
A catalyst speeds up the reaction but does not change the yield, and it is not used up. The backward reaction still happens.
Aincreasing the pressure[1]
A higher pressure gives a higher yield. A higher temperature lowers the yield, a catalyst does not change the yield, and the cooler is needed to remove the ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) [1]
The cracking of crude oil fractions. [1]
So that they are not wasted: they pass over the catalyst again to make more ammonia. [1]
A reaction that can go both forward and backward. [1]
Cburning charcoal[1]
The ash cannot be turned back into charcoal. The other three can go both forward and backward.
NH4Cl(s) ⇌ NH3(g) + HCl(g) [1]
Ammonia has a lower relative molecular mass (17) than hydrogen chloride (36.5) [1]
so ammonia diffuses faster and reaches the litmus paper first. [1]
Ammonium chloride: ammonia and hydrogen chloride combine again where the tube is cooler (both points for the mark). [1]
Acracking of oil fractions[1]
Hydrogen comes from cracking crude oil fractions. Fractional distillation of liquid air is the source of nitrogen.
BHydrogen is obtained from fractional distillation of liquid air.[1]
Nitrogen, not hydrogen, is obtained from liquid air. Hydrogen comes from cracking crude oil fractions.
CIron is used to increase the yield of ammonia.[1]
Iron is a catalyst. It speeds up the reaction but does not change the yield.
Aincrease the pressure to 450 atm[1]
A higher pressure increases the yield. A higher temperature lowers the yield, the gases react in a 1 : 3 ratio, and a catalyst does not change the yield.
BAt 250 °C, the rate of ammonia production is too low.[1]
450 °C is a compromise. At 250 °C the yield is higher, but the reaction is far too slow.
CHigh pressure is used to increase the rate and yield of the reaction.[1]
High pressure gives both a faster rate and a higher yield. Only nitrogen comes from liquid air, iron does not change the yield, and a high temperature lowers the yield.
N2 + 3H2 ⇌ 2NH3: correct balanced equation [1]
Reversible arrow ⇌ [1]
Nitrogen from the fractional distillation of liquid air or hydrogen from the cracking of crude oil fractions. [1]
A reaction that can go both forward and backward at the same time. [1]
A pressure of 250 atm and a temperature of 450 °C. [1]
450 °C, 250 atm and a finely divided iron catalyst. [1]
The reaction between nitrogen and hydrogen is reversible. [1]