Asample of gas with a volume of 2.0 l at stp is found to have a mass of 1.43 g. calculate the molecular mass of this gas. is it possible this gas is methane? why or why not?

15.9gmol⁻¹

The gas could have been methane when we compare the two molecular masses.

Oxygen gas, O₂ also shares this same number for its molecular mass. This would be the reason why it would not be methane.

Explanation:

Given parameters:

Volume of gas at STP = 2.0L or 2.0dm³(1L = dm³)

Mass  of the gas = 1.43g

Unknown:

Molecular mass of the gas = ?

Solution

We can find the number of moles using the mole concept according to the equation below:

          number of moles = ³⁻¹

number of moles =

number of moles = 0.089mol

Using this obtained number of moles, we can derive the molecular mass of the compound by using the relationship between mass and number of moles according to the equation below:

                  molecular mass =

molecular mass =

molecular mass of the gas = 15.9gmol⁻¹

The formula of methane gas is CH₄.

Let's calculate the molecular mass of methane using these atomic masses:

C = 12g and H = 1g

The molecular mass = 12 + (1x4) = 16gmol⁻¹

The gas could have been methane when we compare the two molecular masses.

Oxygen gas, O₂ also shares this same number for its molecular mass. This would be the reason why it would not be methane.

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.