An experiment shows that a 236 mL gas sample has a mass of 0.443 g at a pressure of 740 mmHg and a temperature of 22 ∘C. What is the molar mass of the gas?

49.2 g/mol

Explanation:

Let's first take account of what we have and convert them into the correct units.

Volume= 236 mL x () = .236 L

Pressure= 740 mm Hg x ()= 0.97 atm

Temperature= 22C + 273= 295 K

mass= 0.443 g

Molar mass is in grams per mole, or MM= or MM= . They're all the same.

We have mass (0.443 g) we just need moles. We can find moles with the ideal gas constant PV=nRT. We want to solve for n, so we'll rearrange it to be

n=, where R (constant)= 0.082 L atm mol-1 K-1

Let's plug in what we know.

n=

n= 0.009 mol

Let's look back at MM= and plug in what we know.

MM=

MM= 49.2 g/mol

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be