Answer:
Given:
* Density of unknown gas (d) = 2.25 g/L
* Pressure (P) = 1.00 atm
* Temperature (T) = 25.0 °C = 298.15 K
We need to find:
* Molar mass
To calculate the molar mass, we can use the ideal gas equation:
PV = nRT
Where:
* n = number of moles
* R = universal gas constant = 0.08206 L·atm/(mol·K)
Let's rearrange the ideal gas equation to solve for n:
n = PV / RT
Plug in the given values:
n = (1.00 atm)(2.25 g/L) / (0.08206 L·atm/(mol·K))(298.15 K)
n = 0.100 mol
We know:
mass (m) = density (d) x volume (V)
The volume is 1 L.
So, m = d x V = (2.25 g/L)(1.0 L) = 2.25 g
And we calculated n = 0.100 mol
So, Molar Mass = mass / moles
Molar mass = 2.25 g / 0.100 mol = 22.5 g/mol
