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

where's the diagram?

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.