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Answer :
The pressure in the 6.00 L tank with 32.8 grams of nitrogen gas at 385 K is approximately 7.56 atm.
Given:
Mass of nitrogen gas = 32.8 grams
Molar mass of nitrogen gas (N₂) = 28.02 g/mol (approximately)
Volume of the tank = 6.00 liters
Temperature of the gas = 385 Kelvin
Calculate the number of moles of nitrogen gas:
Number of moles (n) = Mass / Molar mass
Given mass = 32.8 grams and molar mass of nitrogen gas ≈ 28.02 g/mol:
Number of moles (n) ≈ 32.8 g / 28.02 g/mol ≈ 1.171 mol
Now, use the ideal gas law equation to find the pressure (P):
PV = nRT
Given R = 0.0821 L·atm/mol·K and rearranging the equation:
P = nRT / V
Substituting the given values:
P ≈ (1.171 mol) × (0.0821 L·atm/mol·K) × (385 K) / (6.00 L)
P ≈ (45.34251 L·atm) / (6.00 L)
P ≈ 7.56 atm
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