Answer :
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Explanation:
To find the volume occupied by 25.0 g of N2 at STP (Standard Temperature and Pressure), we can utilize the ideal gas law and the concept of molar volume.
Here's the approach:
Ideal Gas Law: The ideal gas law relates pressure (P), volume (V), temperature (T), and moles (n) of a gas through the equation:
PV = nRT
where R is the ideal gas constant (approximately 0.082057 L atm/mol K).
STP Conditions: STP refers to a standard temperature of 273.15 K (0 °C) and a standard pressure of 1 atm.
Molar Volume: At STP, one mole of any ideal gas occupies a volume of 22.4 liters (L). This is a convenient relationship for ideal gas calculations.
Convert mass to moles: We need to determine the number of moles of N2 in 25.0 g. First, find the molar mass of N2, which is 28.0134 g/mol (mass of one mole of N2 molecules).
moles of N2 = mass of N2 / molar mass of N2
= 25.0 g / 28.0134 g/mol
= 0.892 mol (approx.)
Now, let's apply the ideal gas law to find the volume:
V = nRT = (0.892 mol) * (0.082057 L atm/mol K) * (273.15 K)
V ≈ 20.0 L (approx.)
Therefore, 25.0 g of N2 will occupy approximately 20.0 liters at STP.
