To calculate the pressure of nitrogen, we can use the ideal gas law equation, which states that the pressure of a gas is related to its volume, temperature, and the number of moles of gas present. The equation is given as:

PV = nRT

Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin

Given:
Mass of nitrogen = 14 kg
Volume of nitrogen = 0.4 m³
Temperature = 30°C

Converting temperature to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 30 + 273.15 = 303.15 K

Converting mass to moles:
The molar mass of nitrogen (N₂) is 28 g/mol.
Number of moles (n) = mass (kg) / molar mass (kg/mol)
n = 14 kg / 0.028 kg/mol = 500 mol

Substituting the values into the ideal gas law equation:
PV = nRT

P * 0.4 = 500 * R * 303.15

Now we need to determine the value of the ideal gas constant (R). The ideal gas constant is usually given as 8.314 J/(mol·K).

P * 0.4 = 500 * 8.314 * 303.15

Simplifying the equation:
P = (500 * 8.314 * 303.15) / 0.4

Calculating the pressure:
P ≈ 31,223 Pa

Therefore, the pressure of the nitrogen is approximately 31,223 Pa.

Note: It is important to ensure that all units are consistent throughout the calculation. In this case, we converted the temperature to Kelvin and used the SI unit (kg) for mass.

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