40 g of a gas present in a closed container having volume 1.5 L exerts 8.21 atm pressure at 27°C temperature. The molar mass of the gas is

To find the molar mass of the gas, we can use the ideal gas law equation, PV = nRT, where:

P = pressure V = volume n = number of moles R = ideal gas constant T = temperature

First, we need to convert the given values to the appropriate units:

• Pressure (P) = 8.21 atm = 8.21 * 1.01325 * 10^5 Pa (since 1 atm = 1.01325 * 10^5 Pa)
• Volume (V) = 1.5 L = 1.5 * 10^-3 m^3 (since 1 L = 10^-3 m^3)
• Temperature (T) = 27°C = 27 + 273.15 = 300.15 K (since temperature must be in Kelvin)

The ideal gas constant (R) is 8.314 J/(mol*K) in SI units.

We can now substitute these values into the ideal gas law equation to find the number of moles (n):

n = PV/RT = (8.21 * 1.01325 * 10^5 Pa * 1.5 * 10^-3 m^3) / (8.314 J/(mol*K) * 300.15 K)

After calculating the above expression, we get the number of moles (n).

Finally, we can find the molar mass of the gas by dividing the given mass of the gas by the number of moles. The given mass of the gas is 40 g.

Molar mass = mass of gas / number of moles = 40 g / n

After calculating the above expression, we get the molar mass of the gas in g/mol.