What is the volume (in liters) occupied by 49.8 g og HCl at STP

Could you explain the problem

Using ideal gas equation,

P/times V=n/times R/times T

Here,

P denotes pressure

V denotes volume

n denotes number of moles of gas

R denotes gas constant

T denotes temperature

The values at STP will be:

P=1 atm

T=273 K

R=0.0821 atm L mol ⁻¹

Mass of HCl given = 49.8 g

Molar mass of HCl given=36.41

Number of moles of gas, n = / frac{Given mass of the substance}{Molar mass of the substance}

Number of moles of gas, n = / frac{49.8}{36.46}

Number of moles of gas, n = 1.36

Putting all the values in the above equation,

V=/frac{1.36/times 0.0821/times 273}{1}

V=30.6 L

So the volume will be 30.6 L.