Answer:
50 grams of nitrogen gas (N2) has a volume of approximately 41.24 liters at STP.
Step-by-step explanation:
At Standard Temperature and Pressure (STP), which is defined as 0°C (273.15 K) and 1 atmosphere (101.3 kPa) of pressure, one mole of any ideal gas occupies a volume of approximately 22.4 liters.
To find the volume of 50 grams of nitrogen gas (N2) at STP, you need to determine how many moles of nitrogen gas you have and then use the ideal gas law. The molar mass of nitrogen (N2) is approximately 28 grams/mole (14 grams/mole for each nitrogen atom).
First, calculate the number of moles:
Number of moles (n) = Mass (m) / Molar mass (M)
n = 50 g / 28 g/mol ≈ 1.79 moles
Now, use the ideal gas law to find the volume (V):
PV = nRT
Where:
P = Pressure (at STP, it's 1 atm)
V = Volume (what we want to find)
n = Number of moles (1.79 moles)
R = Ideal gas constant (approximately 0.0821 L·atm/mol·K)
T = Temperature in Kelvin (273.15 K)
Now, plug in these values:
(1 atm) * V = (1.79 moles) * (0.0821 L·atm/mol·K) * (273.15 K)
V = (1.79 moles) * (0.0821 L·atm/mol·K) * (273.15 K) / (1 atm)
V ≈ 41.24 liters
So, 50 grams of nitrogen gas (N2) has a volume of approximately 41.24 liters at STP.