According to le châtelier's principle, how will a decrease in concentration of a reactant affect the equilibrium system? shift it toward the products shift it toward the reactants shift it toward the side with higher total mole concentration shift it toward the side with lower total mole concentration

Shift it toward the products

Explanation:

According to Le Chatelier's principle, changes to an system at equilibrium will result in a predictable shift that will counteract the change causing it.Therefore, adding additional reactant to a system will shift the equilibrium to the right, towards the side of the products.Conversely, reducing the concentration of any product will also shift equilibrium to the right to the side of the reactants.

For cyclohexane compounds drawn in a chair conformation:   -axial bonds are vertical  -equatorial bonds are parallel to two bonds within the ring.  thus, as i assume the chair conformation is drawn:   -the x group is in an axial position, as are the five other vertical bonds.  -three axial bonds are on the top face of the ring  -the other three axial bonds are on the bottom face  the position of the second substituent on each ring carbon is equatorial.  gauche groups must be on an adjacent carbon such as carbon 6 and carbon 2, and also gauche groups are rotated by 60 degrees relative to each other.  drawing the newman projections for c1–c2 and c1–c6 aids in visualizing the groups that are gauche to the y group on c1.  click this link and watch some academic videos that may you more understand the topic