Consider the reaction 2NO2(g) ⇌ N2O4(g) For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. a. PNO2 = PN2O4 = 1.0 atm b. PNO2 = 0.21 atm, PN2O4 = 0.50 atm c. PNO2 = 0.29 atm, PN2O4 = 1.6 atm

The effects of varying pressure change is outlined below:

Explanation:

Le Chatelier’s principle implies that equilibrium will always shift to counteract any changes in the reaction system. In a gaseous system as this, an increment in pressure shifts an equilibrium to the side of the reaction with the fewer number of moles of gas, or higher atmospheric pressure, and vice versa. If the number of moles of gas is the same on both sides of the reaction, pressure has no effect.

Pressure, P of NO2 = P of N2O4: reaction equilibrium remains the samePressure, P of NO2 is less than N204: reaction shifts to favour reactantPressure P of NO2 is less than N2O4: Reaction shifts to favour reactant

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