3
A
3of 3
0.030
0.040
4.8 x 10-8
6.4 x 10-8
Chemical Change Assignment 2
SECTION 4 (AC4.1 / AC4.2) (A) For the following reactions, determine the equilibrium constant equation. You must show your workings within your submission.
1) CO2(g) + H2(g) ,=’ CO(g) + H20(g) 2) 2N0(g) + 2H2(g) ,’=” N2(g) + 2H20(g) 3) Cu(s) + 2Ag+(g) ,n’ Cu24-(g) + 2Ag(s) 4) H2(g) + 12(g) ,=’ 2HI(g)
(B) Read the following relating to the Haber process:
“The raw materials for this process are hydrogen and nitrogen. Hydrogen is obtained by reacting natural gas – methane – with steam, or through the cracking of oil.
Nitrogen is obtained by burning hydrogen in air. Air is 80% nitrogen; nearly all the rest is oxygen. When hydrogen is burned in air, the oxygen combines with the hydrogen, leaving nitrogen behind. Nitrogen and hydrogen will react together under these conditions:
• A high temperature – about 4500C • A high pressure – about 200 atmospheres (200 times normal pressure) • An iron catalyst”
The chemical reaction which occurs during the Haber process is: Nitrogen + Hydrogen ,’ Ammonia N2(g) + 3H2(g) ,’ 2NH3(g)
1. Explain Le Chatelier’s principle.
2. Use Le Chatelier’s principle to explain what would happen if you raised the temperature of this reaction.
3. Use Le Chatelier’s principle to explain what would happen if you increased the pressure of this reaction.
4. Use Le Chatelier’s principle to explain what would happen if you increased the concentration of Nitrogen at the start of the reaction.
Your response for this question should be a maximum of 500 words.
Chemical Change Assignment 3
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