Question

Reactions can have a wide range of yields. They can produce anything from fractions of percents all the way to almost exactly 100%. The reason that they almost never reach 100% is that almost all reactions are reversible, and once a certain concentration of product is reached, the reaction is no longer favorable.

Hypothesize a way that you could force a reaction to reach 100%. Explain why it would work and why the reverse reaction wouldn’t occur.

Answer 1

According to Le-chatlier principle, If a reaction in equilibrium is subjected to a change in concentration, temperature, pressure or volume,then equilibrium will shift in a direction to undo the effect of change.

So, if we remove the product time to time from this reaction, then reaction will move forward to produce more products as reaction takes place in a closed vessel

For example

A+B C

Here C can be in gaseous phase or liquid. SO if C is a gas and it escapes then their is no C to react back and give reactants. And According to Le-Chatlier Principle, it will give More C

And If C is a liquid then it can be removed by distillation .

In this way we can get 100 % product or forward reaction is forced to reach 100%