What is the volume of nitrogen in a vessel under a pressure of 2 * 10 ^ 5 Pa at a temperature of 30 degrees C.

What is the volume of nitrogen in a vessel under a pressure of 2 * 10 ^ 5 Pa at a temperature of 30 degrees C. The mass of nitrogen is 4.5 * 10 ^ -3 kg. The molar mass is 0.028 kg / mol?

Given:

m = 4.5 * 10 ^ -3 kg is the mass of nitrogen;

M = 0.028 kg / mol is the molar mass of nitrogen;

P = 2 * 10 ^ 5 Pa – nitrogen pressure;

T = 30 degrees Celsius = 303 degrees Kelvin – nitrogen temperature.

R = 8.31 J / mol * K – gas constant.

It is required to determine the volume V (m ^ 3) occupied by nitrogen.

According to the Cliperon-Mendeleev law:

V = m * R * T / (M * P) = 4.5 * 10 ^ -3 * 8.31 * 303 / (0.028 * 2 * 10 ^ 5) =

= 11.3 / 5600 = 0.002 m ^ 3 or 2 liters.

Answer: nitrogen occupies a volume equal to 0.002 m ^ 3 (2 liters).




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