Step-by-step explanation:
To find the mass of a gas at STP (Standard Temperature and Pressure), we need to use the ideal gas law, which states:
PV = nRT
Where:
P = Pressure (at STP, it is 1 atm)
V = Volume (2.15 liters in this case)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (at STP, it is 273.15 K)
Rearranging the equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (1 atm) * (2.15 L) / [(0.0821 L·atm/(mol·K)) * (273.15 K)]
n = 2.15 / 22.414
n ≈ 0.096 moles
Now, to find the mass of N2 gas, we need to multiply the number of moles by the molar mass of N2.
The molar mass of N2 is approximately 28.02 g/mol.
Mass = n * molar mass
Mass = 0.096 moles * 28.02 g/mol
Mass ≈ 2.689 g
Therefore, the mass of 2.15 liters of N2 gas at STP is approximately 2.689 grams.