1. Convert Units
* Volume: 347 mL = 0.347 L (1 L = 1000 mL)
* Pressure: 6680 torr = 8.82 atm (1 atm = 760 torr)
* Temperature: 27 °C = 300 K (K = °C + 273.15)
2. Ideal Gas Law
The ideal gas law is:
PV = nRT
Where:
* P = Pressure (in atm)
* V = Volume (in L)
* n = Number of moles
* R = Ideal gas constant (0.0821 L·atm/mol·K)
* T = Temperature (in K)
3. Solve for n
Rearrange the ideal gas law to solve for 'n':
n = PV / RT
4. Plug in Values
n = (8.82 atm)(0.347 L) / (0.0821 L·atm/mol·K)(300 K)
5. Calculate
n ≈ 0.124 moles
Answer: Approximately 0.124 moles of nitrogen gas will occupy that volume under those conditions.
