1. Convert Units
* Temperature: Convert Celsius to Kelvin:
- K = °C + 273.15
- K = -19.0°C + 273.15 = 254.15 K
* Pressure: No conversion needed, as atmospheres are the standard unit for pressure in the ideal gas law.
2. The Ideal Gas Law
The ideal gas law is:
PV = nRT
where:
* P = Pressure (in atmospheres)
* V = Volume (in liters)
* n = Number of moles
* R = Ideal gas constant (0.0821 L·atm/mol·K)
* T = Temperature (in Kelvin)
3. Solve for Volume (V)
Rearrange the equation to solve for V:
V = (nRT) / P
4. Plug in the Values
V = (880 mol * 0.0821 L·atm/mol·K * 254.15 K) / 2.75 atm
5. Calculate the Volume
V ≈ 6537.6 L
Therefore, the approximate volume of the 880 mol gas sample at -19.0°C and 2.75 atm is about 6537.6 liters.
