Answer
option b) 60.1 g/mol is correct answer.
Work Step by Step
Here in the question we have given
density of the gas (d) = 1.963 g/L , pressure (P) = 1.00 atm , Temperature (T) = 100$^{\circ}$C = 373 K and value of gas constant (R) = 0.08206 L atm k−1mol−1
Now, we have to determine the molar mass of gas
the ideal gas equation is PV=nRT from this relation we can get the new relation
i;e
PM=dRT
molar mass (M) = $\frac{dRT}{P}$= $\frac{1.963 g/L\times 0.08206 L \space atm\space K^{-1}\space mol^{-1}\times\space373 K}{1.00 atm}$ = 60.10 g/mol
Molar mass of the gas is 60.1 g/mol
therefore option b) is correct
