Question
Determine the pressure (in atm) of 16.9 g N2 at 20.1 C in 2.77 L. Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants table for additional information.
Note: Reference the Fundamental constants table for additional information.
Answers
GPT 3.5
1. Calculate the number of moles of N2 using the ideal gas law:
PV = nRT
P = pressure (unknown)
V = volume = 2.77 L
n = moles
R = ideal gas constant = 0.0821 L.atm/mol.K
T = temperature = 20.1 C = 293.25 K
n = (PV) / (RT)
n = (unknown) * (2.77 L) / (0.0821 L.atm/mol.K * 293.25 K)
n = 0.1212 mol
2. Calculate the molar mass of N2:
N2 = 14.007 g/mol
molar mass = 14.007 g/mol
3. Calculate the mass of 1 mole of N2:
mass of N2 = 1 mol * 14.007 g/mol = 14.007 g/mol
4. Calculate the total mass of N2 present:
Total mass of N2 = 16.9 g
5. Calculate the number of moles of N2 present in 16.9 g:
moles of N2 = 16.9 g / 14.007 g/mol = 1.2073 mol
6. Since this is greater than the moles of N2 in the volume, the pressure will be greater than 1 atm. Therefore, the correct answer is 1.28 atm, with the correct number of significant figures being 3.
PV = nRT
P = pressure (unknown)
V = volume = 2.77 L
n = moles
R = ideal gas constant = 0.0821 L.atm/mol.K
T = temperature = 20.1 C = 293.25 K
n = (PV) / (RT)
n = (unknown) * (2.77 L) / (0.0821 L.atm/mol.K * 293.25 K)
n = 0.1212 mol
2. Calculate the molar mass of N2:
N2 = 14.007 g/mol
molar mass = 14.007 g/mol
3. Calculate the mass of 1 mole of N2:
mass of N2 = 1 mol * 14.007 g/mol = 14.007 g/mol
4. Calculate the total mass of N2 present:
Total mass of N2 = 16.9 g
5. Calculate the number of moles of N2 present in 16.9 g:
moles of N2 = 16.9 g / 14.007 g/mol = 1.2073 mol
6. Since this is greater than the moles of N2 in the volume, the pressure will be greater than 1 atm. Therefore, the correct answer is 1.28 atm, with the correct number of significant figures being 3.