How many molecules of CH4 are present in a 1.00L flask at 300K and 4.00 atm?

0.964× 10²³ molecules

Explanation:

Given data:

Number of molecules of CH₄ = ?

Volume = 1.00 L

Temperature = 300 K

Pressure = 4.00 atm

Solution:

First of all we will calculate the number of moles of CH₄ from ideal gas equation.

PV = nRT

n = PV/RT

R = general gas constant = 0.0821 atm. L/mol.K

n = 4.00 atm× 1.00 L  /  0.0821 atm. L/mol.K × 300 k

n = 4.00 atm.L / 24.63  atm. L/mol

n = 0.16 mol

Now we will determine the number of molecules by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

1 mole of CH₄ = 6.022 × 10²³ molecules of CH₄

0.16 mol  ×  6.022 × 10²³ molecules  / 1 mol

0.964× 10²³ molecules

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