RoseMarie Gallagher and Paul Ingram Solutions for Chapter: Energy Changes, and Reversible Reactions, Exercise 7: Q

The reaction between nitrogen and hydrogen is reversible. This causes a problem for the ammonia factory. Why?

What is Le Chatelier‘s principle? Write it down.

In manufacturing ammonia, explain why: high pressure is used.

In manufacturing ammonia, explain why: ammonia is removed.

Sulphur dioxide (${\mathrm{SO}}_2$) and oxygen react exothermically to form sulphur trioxide (${\mathrm{SO}}_3$). The reaction is reversible. Write the symbol equation for this reaction.

Sulphur dioxide $\left({\mathrm{SO}}_2\right)$ and oxygen react exothermically to form sulphur trioxide $\left({\mathrm{SO}}_3\right)$. The reaction is reversible. What happens to the yield of sulphur trioxide if you: increase the pressure?

Sulphur dioxide $\left({\mathrm{SO}}_2\right)$ and oxygen react exothermically to form sulphur trioxide $\left({\mathrm{SO}}_3\right)$. The reaction is reversible. What happens to the yield of sulphur trioxide if you: raise the temperature?