Determine the pressure of nitrogen (N2) in the cylinder at a temperature of 280 K. The density of nitrogen is 100g / m3.

Let’s turn to the Mendeleev-Clapeyron equation: p * v = m / M * R * T, p – pressure, v – volume, m – gas mass, M – molar mass, R – universal gas constant, T – temperature. Dividing this equation by v we get:

p = 1 / M * (m / v) * R * T.

m / v is the density of the substance ρ. Then:

p = 1 / M * ρ * R * T.

The molar mass of nitrogen is 28 * 10 ^ (- 3) kg. We substitute the known values into the resulting formula:

p = 1/28 * 10 ^ (- 3) * 0.1 * 8.31 * 280 = 8.31 * 10 ^ (3) Pa = 8.31 KPa.

Answer: the pressure is 8.31 kPa.