How many liters of liquid nitrogen are produced when 360.0 L of nitrogen gas is liquified at 77.36 kl
I don't see a pressure or a density.
Use PV = nRT assuming you have a pressure somewhere and solve for = number of mols.
Then find the density of liquid N2 at that temperature (I don't know what K| stands for) and use volume = mass/density.
To find out how many liters of liquid nitrogen are produced when 360.0 L of nitrogen gas is liquefied, we need to know the density of nitrogen gas and the process of liquefaction.
The density of nitrogen gas is typically around 1.25 kg/m³ at room temperature and pressure (or 25°C and 1 atm). However, since the temperature and pressure in your question are specified, we need to use the values given.
To perform the calculation, we also need to convert kiloliters (kl) to liters. Since there are 1,000 liters in a kiloliter, 77.36 kl is equal to 77.36 × 1,000 = 77,360 liters.
Now, let's assume that the density of the nitrogen gas at the given temperature and pressure is still approximately 1.25 kg/m³. We can convert this to grams per liter (g/L) by multiplying by 1,000 to get 1,250 g/L.
To find the mass of nitrogen gas, we multiply the density by the volume:
Mass of nitrogen gas = density × volume = 1,250 g/L × 360.0 L = 450,000 g.
Since liquid nitrogen is denser than nitrogen gas, we need to use the density of liquid nitrogen to calculate its volume. The density of liquid nitrogen is approximately 808 kg/m³, which is equal to 808 g/L.
To find the volume of liquid nitrogen, we divide the mass by the density:
Volume of liquid nitrogen = mass / density = 450,000 g / 808 g/L = 556.93 L.
Therefore, when 360.0 L of nitrogen gas at the given temperature and pressure is liquefied, approximately 556.93 liters of liquid nitrogen are produced.