Ammonia (NH3\text{NH}_3NH3) is made in industry by reacting nitrogen (N2\text{N}_2N2) with hydrogen (H2\text{H}_2H2) at a temperature of 450∘C450^\circ\text{C}450∘C and a pressure of 200 atm200\text{ atm}200 atm. Under these conditions, the percentage yield of ammonia is about 15%. The equation for the reaction is:
N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ/mol \text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightleftharpoons 2\text{NH}_3\text{(g)} \quad \Delta H = -92\text{ kJ/mol} N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ/molState what the symbols ⇌ \rightleftharpoons\,⇌ and ΔH \Delta H\,ΔH represent.
Name the catalyst used in this industrial process.
Predict the effect on the yield of ammonia if the reaction is carried out at a temperature lower than 450∘C450^\circ\text{C}450∘C, but at the same pressure of 200 atm200\text{ atm}200 atm. [assume reaction reaches equilibrium] Give a reason for your answer.
Predict the effect on the yield of ammonia if the reaction is carried out at a pressure lower than 200 atm200\text{ atm}200 atm, but at the same temperature of 450∘C450^\circ\text{C}450∘C. [assume reaction reaches equilibrium] Give a reason for your answer.
One method of obtaining hydrogen is by reacting methane from natural gas with steam. Hydrogen can also be made by the electrolysis of acidified water. The equation for the reaction is:
2H2O(l)→electricity2H2(g)+O2(g) 2\text{H}_2\text{O(l)} \xrightarrow{\text{electricity}} 2\text{H}_2\text{(g)} + \text{O}_2\text{(g)} 2H2O(l)electricity2H2(g)+O2(g)State the type of reaction taking place.
Suggest why it may be necessary, in the future, to make hydrogen using this reaction rather than from natural gas.
