It is found that 250 ml of gas at stp has a mass of .675 g what is the molar mass

The molecular weight of the 250ml of gas found at STP has a molar mass of 60.81 g/mol.

According to the ideal gas equation:

PV= nRT

P = pressure = 1 atm at STP

V= volume = 250 ml = 0.25 L

n = moles

R = constant = 0.0821 atmp

T = temperature = 273.15 K

moles can be written as

PV =

1 0.25 = 0.0821 273.15

0.25 = 22.425

molecular weight =

molecular weight = 60.81 g/mol.

The molecular weight of the gas found at STP has a molar mass of 60.81 g/mol.

For more information about the molar mass, refer to the link:

link

61.3 g/mol  

Step-by-step explanation:

We can use the Ideal Gas Law to solve this problem:

       pV = nRT

Since n = m/M, the equation becomes

       pV = (m/M)RT     Multiply each side by M

    pVM = RT              Divide each side by RT

         M = (mRT)/(pV)

Data:

m = 0.675 g

R = 0.0.083 14 bar·L·K⁻¹mol⁻¹

T = 0 °C = 273.15 K

p = 1 bar

V = 250 mL = 0.250 L

Calculation:

M= (0.675 × 0.083 14 × 273.15)/(1 × 0.250)

M= 15.33/0.250

M= 61.3 g/mol

it is the most commonly accepted one