what is the pressure (in torr) inside a 4.0 liter flask at 24°c of 7.2 grams of nitrogen gas (remember that nitrogen gas is diatomic)?

1190.2 Torr

Explanation:

Data Given:

Volume of a nitrogen gas ( V )= 4.0 L

temperature of a gas ( T ) = 24 °C

Convert °C  to K

T = °C + 273

T = 24 + 273 = 297 K

mass of nitrogen gas (m) = 7.2 g

Pressure of a gas ( P ) =? in Torr

Solution:

Formula to be used

            PV= nRT . . . . . . .(1)

As we Know

           n= m/M

So, the equation 1 can be written as

      PV = (m/M)RT

Rearrange the above formula

       P = (m/M)RT / V . . . . . . . . . . (2)

Where

R is ideal gas constant

R = 62.37 L Torr mol⁻¹ K⁻¹

M = molar mass of N₂

molar mass of N₂ = 2(14) = 28 g/mol

m = mass of N₂ gas

Put values in equation 1

           P = (m/M)RT / V

          P = (7.2 g / 28 g/mol) 62.37 L Torr mol⁻¹ K⁻¹ x 297 K / 4.0 L

           P = 0.257 mol x 62.37 L Torr mol⁻¹ K⁻¹ x 297 K /4.0 L

           P = 4761 L Torr / 4.0 L

           P = 1190.2 Torr

Pressure of gas (N₂) = 1190.2 Torr

108

explanation:

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it is stable as it is in group 0 which have full outer shells of electrons