Equilibrium and Kinetics
At this point of advancements in science, chemists have a good understanding of the kinetics of reactions. They can predict the effects of changes in pH, temperature, and concentration in chemical reactions.
In a cylinder, there is a reaction mixture of hydrogen and iodine. The hydrogen and the iodine react to form hydrogen iodide.
The industrial production of ammonia is done by a process called Haber process. The reaction occurs as shown below, and is usually done in the presence of an iron catalyst.
ΔH = –92kJ
A student researcher conducted experiments on the effects of changes in the conditions on reactions. The student did the experiments with Reaction 2, by increasing the pressure on the cylinder where the reaction mixture was present. Which of the following are completely true regarding the experiment?
I. The reaction will shift toward the right, because there are more moles on the product side.
II. The reaction will shift toward the left, because there are more moles on the reactant side.
III. The reaction will have increased production of ammonia, because there are more moles on the reactant side.
|D|| II & III|
In Reaction 2, a pressure change will affect the reaction. Here, the pressure is increased and that will increase the forward reaction. In other words, the reaction shifts to the right. Item I does says that the reaction shifts to the right. But for the wrong reason. According to the equation, we have more moles on the reactant side. So item I is not fully correct. Item II is also ruled out because the reaction shifts to the right. Item III makes perfect sense.