How many liters of CO2 are present in a sample with 1.5 x 1022 particles?

Explanation:

We can convert particles to moles in 3 steps:

1. Convert Particles to Moles

First, we must convert particles to moles. 1 mole of any substance contains the same number of particles: 6.022*10²³ or Avogadro's Number. For this problem, we have particles of carbon dioxide or CO₂. We can make a ratio.

Since we are converting 1.5*10²² particles to moles, we multiply the ratio by that value.

Flip the ratio. It remains equivalent, but the units of particles of carbon dioxide can cancel.

2. Convert Moles to Liters

There are 22.4 liters in 1 mole of any gas. Let's set up another ratio.

Multiply by the number of moles we calculated.

The units of moles of carbon dioxide cancel.

3. Round

The original measurement of particles (1.5*10²²)  has 2 significant figures (1 and 5). Our answer must have the same number. For the number we calculated, that is the hundredth place.

The 7 in the thousandth place (0.55795416805) tells us to round the 5 in the hundredth place up to a 6.

1.5*10²² particles of carbon dioxide is equal to 0.56 liters of carbon dioxide.

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 

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