By what factor does the gas temperature change if the volume is doubled and the pressure is tripled?

If the volume is doubled and the pressure is tripled, the temperature changes by a factor of 6.

Explanation:

Since, for ideal gases the temperature is in direct relation to the volume and the pressure, you can predict that if the volume is doubled and the pressure is tripled the effect on the temperature will be 3 × 2 = 6 times.

You can prove it using the combined law of gases:

P₁ V₁ /T₁ = P₂ V₂ / T₂

Where the letters P denote absolute pressures, the letters T denote temperature measured in absolute scale, and the letters V denote volume.

The changes given may be written it this way:

V₂ = 2 × V₁ = 2V₁P₂ = 3 × P₁ = 3P₁

Then, you can write T₂ in terms of the other variables:

T₂ = (P₂ V₂  T₂) / (P₁ V₁) = 3P₁ 2V₁ T₂ / (P₁V₁)

Cancel the common factors P₁ and V₁

T₂ = 6 T₁

Which proves that the final temperature is 6 times the initial temperature.

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