FERTILISERS - Haber Process and Le Chatelier’s Effects on Pressure and Temperature

Oct 14, 2026

Uploaded by hdkawk

Instructional questions and interactive gap-fill explanations on fertilisers chemistry, focusing on the Haber Process for producing ammonia. Covers nitrogen’s importance, purpose of the process, balanced reversible equation, uses of ammonia, equilibrium conditions and characteristics, and the role of catalysts. Includes True/False and matching activities for equilibrium concepts, then detailed Le Chatelier’s effects of pressure (increased, decreased, optimum) and temperature (heating) on forward and reverse reaction rates, reactant/product amounts, and the equilibrium constant Kc.

LanguageEnglish

CategoryExam

FormatPDF

Pages5

Reading Time13 min

AccessFree to download

FERTILISERS

Haber Process

Le Chatelier: Effect of pressure

Le Chatelier: Effect of temperature

FERTILISERS Overview 1 Why is nitrogen important to plants? 3 Complete to summarise the industrial processes: | Process | Reactants | Products of step 1 | Products of step 2 | Final products | | --- | --- | --- | --- | --- | | Haber | | not applicable | | | | Ostwald | | | | | | Contact | | | | | Haber Process 4 What is the purpose of the Haber Process? To produce from and . 5 Write a balanced equation for the Haber Process's reversible reaction: + 6 Name some uses of ammonia. 7 Name two conditions which must be met for a reaction to reach equilibrium. 8 Name two characteristics of equilibrium. 9 In the Haber Process an iron oxide catalyst is usually used. Ruthenium can also be used. What does a catalyst do in a reaction, and how does it do this? 􀂈 Creative Commons BY-NC-SA CHEMICAL INDUSTRIES RESOURCE PACK 􀀙 10 Circle the correct option (True / False) for each of the following: i A catalyst speeds up the Haber Process's forward reaction more than the reverse. [True / False] ii A catalyst will cause more product to be formed. [True / False] iii A catalyst will decrease the time it takes to reach equilibrium because it speeds up both forward and reverse reactions. [True / False] iv A catalyst speeds both forward and reverse reactions equally. [True / False] 11 Link each element from Column A with its corresponding element in Column B. Write the letter from A next to each item in B in the last column. Column A Column B A a dynamic equilibrium absorbs heat b endothermic a measure of the average kinetic energy of particles c exothermic disturbs equilibrium, favours increased crowding: more molecules d Le Chatelier's principle 273 K and 101,3 kPa e decrease in pressure disturbs equilibrium, favours exothermic reaction f increase in pressure releases heat g removing heat a state in which forward and reverse reactions occur at equal rates h adding heat force per area, in gases related to rate of particle collisions i temperature disturbs equilibrium, favours decreased crowding, fewer molecules j pressure disturbs equilibrium, favours endothermic reaction k STP when a system which is in equilibrium is disturbed, it will respond in such a way as to counteract the disturbance Le Chatelier: Effect of pressure 12 Complete the explanation by filling the gaps or choosing from the options. Do this before, or after, but not during, watching the animations. Mark during re-watching. Increased pressure According to principle, when a system which is in equilibrium is disturbed, it will respond in such a way as to the disturbance. An increase in pressure [de/in]creases the crowding of gaseous molecules. The system will respond by [de/in]creasing their crowding. Crowding is decreased in gases when [fewer/more] molecules are formed. In the Haber Process the [forward/reverse] reaction makes fewer molecules than the [forward/reverse] reaction. In the forward reaction molecules of ammonia are made from every molecules of reactants ( ~~ ~~ N2 and ~~ ~~ H2 molecules) . Consequently, an increase in pressure equilibrium for a while by making the [forward/reverse] reaction occur ata higher rate than the [forward/reverse] reaction. This causes [more/less] ammonia to be formed and [more/less] nitrogen and hydrogen. After a while a new dynamic equilibrium is reached. The rates of forward and reverse reactions are again to one another, and the amounts of reactants and products will [change/remain constant] . However, compared to before the pressure was applied, there will now be [more/less] ammonia present at equilibrium. The equilibrium constant value, Kc, however, will be [higher than/lower than/the same as] it was in the original equilibrium. 􀀚 CHEMICAL INDUSTRIES RESOURCE PACK 􀂈 Creative Commons BY-NC-SA Decreased pressure Decreasing pressure [de/in]creases the crowding of gaseous molecules. The system will respond by

FAQs

Why is nitrogen important to plants in fertiliser chemistry?

Nitrogen is an essential nutrient for plant growth, so fertilisers support plant nitrogen requirements.

What is the purpose of the Haber Process?

The Haber Process is used to produce ammonia from nitrogen and hydrogen.

How does changing pressure affect equilibrium in the Haber Process?

Increasing pressure shifts the equilibrium toward the side that forms fewer gas molecules, increasing ammonia at equilibrium; decreasing pressure shifts it toward forming more gas molecules, reducing ammonia.

Oct 14, 2026

Uploaded by hdkawk