Question

Topic Factors Affecting Reaction Rates LaTeX: A+B\Leftrightarrow C+DA + B ⇔ C + D 1. Using the reaction above, which way will the reaction move if we add more "A+B?" 2. Using the reaction above, which way will the reaction move if we remove "A+B?" 3. Using the reaction above, which way will the reaction move if we add more "C+D?" 4. Using the reaction above, which way will the reaction move if we remove "C+D?"

Answer 1

A +B <=> C +D

As we can see it's a reversible reaction. We can say the reaction A+ B -> C + D is the forward reaction and C + D -> A + B is the backward reaction. The forward reaction takes place from left to right direction and hence the reactants on the left side reacts to form products which are written in the right side of the reaction.

Similarly, in the backward reaction the products produced in the forward reaction acts as reactants and written in the right side of the reversible reaction and the products produced in the backward reaction are the reactants of the forward reaction and are written in the left side of the reversible reaction.

1. If we will add more A +B than the concentration of the reactants increase and the reaction will takes place in forward direction.

2. If we will remove A +B , than the concentration of the reactants decreases than the concentration of the products and the reaction takes place in the backward direction.

3. On adding more C + D to the reaction, the concentration of the products increases as compare to the concentration of the reactants and the reaction will move in the backward direction.

4. When C + D will be removed from the reversible reaction, the concentration of the products is less than the concentration of the reactants and the reaction takes place in the forward direction.

It is should be noted that, in a reversible reaction, the reaction always takes place in a direction in which the concentration is less as compare to the other side. Hence when the concentration of the reactants is more than the products, the reaction takes place in the forward direction and when the concentration of the products is more than the reactants, the reaction takes place in the backward direction.