A sample of an unknown compound is vaporized at . The gas produced has a volume of at a pressure of

Explanation:

Given:

T = 190 °C

= 190 + 273

= 463 K

V = 2420 ml

= 2.42 l = 0.00242 m^3

P = 1 atm

= 1.01325 × 10^5 N/m^2

M = 2.04 g

Using ideal gas law,

P × V = n × R × T

Number of moles, n = (1.01325 × 10^5 × 0.00242) ÷ 8.314 × 463

= 0.0637 mole

Molar mass = mass/no of moles

= 2.04/ 0.0637

= 32.025 g/mol