A quantity of N2 occupies a volume of 1.5L at 300K and 1.2atm. The gas expands to a volume of 3.1L as the result of a change in both temperature and pressure.

Find the density of the gas at these new conditions.

The density of the nitrogen gas at the new condition is 1.35 g/L.

The given parameters;

The number of moles of the gas in the new condition is calculated as follows;

The mass of the nitrogen gas is calculated as;

The density of the nitrogen gas is calculated as follows;

Thus, the density of the nitrogen gas at the new condition is 1.35 g/L.

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0.661g/L

Explanation:

T = 300K

P = 1.2atm

V = 1.5L

R = 0.082atm.L/K /mol

n =?

From the ideal gas equation PV = nRT

n = PV /RT = (1.2x1.5)/(300x0.082)

n = 0.0732mol

Molar Mass of N2 = 28g/mol

Mass conc. = n x molar Mass

Mass conc = 0.0732 x 28

Mass conc of N2 = 2.0496g

Volume = 3.1L

Mass = 2.0496g

Density =?

Density = Mass /volume

Density = 2.0496/3.1

Density = 0.661g/L

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this chemical reaction releases energy in the form of light and heat. chemical energy is the potential energy stored in the arrangement of atoms within molecules. breaking chemical bonds requires energy, while forming new chemical bonds releases energy.

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because it does not have the potential to be entirely used up