What is the molar mass of a gas (96.0 g) in a 25.0 L container at 27.0 °C? The pressure inside the container is 3.04E5 Pa.

PV=nRT

n=96/molmass * PV/RT

solve for molmass

Silver has a density of 10.5 g/cm3 and crystallizes in a face-centered cubic unit cell (see below). Calculate the atomic radius (in Å) of Silver.

To calculate the molar mass of a gas, you can use the ideal gas law equation, PV = nRT, where P represents the pressure, V represents the volume, n represents the number of moles, R represents the ideal gas constant, and T represents the temperature in Kelvin.

First, let's convert the given temperature from Celsius to Kelvin by adding 273.15:
T = 27.0 °C + 273.15 = 300.15 K

Next, let's rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT

Now, let's substitute the given values into the equation:
P = 3.04E5 Pa
V = 25.0 L
R = 8.314 J/(mol·K)
T = 300.15 K

n = (3.04E5 Pa) * (25.0 L) / (8.314 J/(mol·K) * 300.15 K)

To simplify the units, we can convert Pa·L to J using the conversion factor 1 L·atm = 101.325 J:
n = (3.04E5 Pa * 25.0 L) / (8.314 J/(mol·K) * 300.15 K) * (1 L·atm / 101.325 J)

Now, let's calculate the value of n:
n ≈ 9.38 mol

Finally, to calculate the molar mass of the gas, we can divide the given mass (96.0 g) by the number of moles (n):
molar mass = mass / moles

molar mass = 96.0 g / 9.38 mol

molar mass ≈ 10.25 g/mol

Therefore, the molar mass of the gas in the 25.0 L container at 27.0 °C and a pressure of 3.04E5 Pa is approximately 10.25 g/mol.