Question

G a sealed container holds 0.020 moles of nitrogen (n2) gas, at a pressure of 1.5 atmospheres and a temperature of 290 k. the atomic mass of nitrogen is 14.0 g/mol. the boltzmann constant is 1.38 × 10-23 j/k and the ideal gas constant is r = 8.314 j/ mol · k = 0.0821 l · atm/mol · k. the mass density of the gas is closest to

Answer 1

Density is a value for mass, such as kg, divided by a value for volume, such as m3. Density is a physical property of a substance that represents the mass of that substance per unit volume. For gases we use the ideal gas equation to solve for density. We do as follows: PV = nRT PV = mRT / MM Density = m/V = PMM / RT From the given conditions of the nitrogen gas, we substitute the given values as follows: Density = PMM / RT Density = 1.5 atm ( 28.02 g / mol) / (0.08205 L-atm / mol-K) (290 K) Density = 1.77 g/L Therefore, the density of the gas is 1.77 g per liter.

Answer 2

Explanation:

The given data is as follows.

        n = 0.020 moles,    P = 1.5 atm

        T = 290 K,      molar mass of nitrogen = 14.0 g/mol

         R = 8.314 J/mol,         d = ?

It is known that  the relation between density, pressure, and temperature is as follows.

                 P = $\frac{d}{\text{molar mass}} \times RT$

Putting the given values into the above relation and calculate the density as follows.

              P = $\frac{d}{\text{molar mass}} \times RT$

             1.5 atm = $\frac{d}{14.0 g/mol} \times 8.314 \times 290 K$

                    d = $\frac{1.5 atm \times 14.0 g/mol}{8.314 L atm/mol K \times 290 K}$

                      = $1.74 \times 10^{-4}$ g

Thus, we can conclude that density of the given gas is $1.74 \times 10^{-4}$ g.