Question

Determine the pressure (in mmHg) of 18.6 g N2 at 16.6 C in 5.60 L. Be sure your answer has the correct number of significant figures.

Note: Reference the Fundamental constants and Conversion factors for non-SI units tables for additional information.

Answer 1

To determine the pressure of the N2 gas, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.08206 L.atm/mol.K)
T = temperature (in Kelvin)

First, we need to determine the number of moles of N2 gas:
molar mass of N2 = 28.0134 g/mol

Number of moles = mass / molar mass
Number of moles = 18.6 g / 28.0134 g/mol
Number of moles = 0.663 mol

Next, convert the temperature to Kelvin:
T (K) = 16.6 C + 273.15
T (K) = 289.75 K

Now, we can plug the values into the ideal gas law equation:

P(5.60 L) = (0.663 mol)(0.08206 L.atm/mol.K)(289.75 K)

P(5.60 L) = 12.44 atm

Convert atm to mmHg:
1 atm = 760 mmHg

P = 12.44 atm * 760 mmHg/atm
P = 9464.40 mmHg

Therefore, the pressure of 18.6 g N2 at 16.6 C in 5.60 L is 9464 mmHg (or 9500 mmHg if we consider the correct number of significant figures).