2.00 g of an unknown gas at STP fills a 500. mL flask. What is the molar mass of the gas?

The molar mass of the unknown gas in the 500 mL flask at stp is 89.7 g/mol

We'll begin by calculating the number of mole of the gas that occupied 500 mL at stp.

Recall at stp:

22400 mL = 1 mole of the gas

Therefore,

500 mL = 500 / 22400 = 0.0223 mole of gas.

Finally, we shall determine the molar mass of the gas. This can be obtained as follow:

Mass of gas = 2 g

Mole of gas = 0.0223 mole

Molar mass = mass / mole

Molar mass of gas = 2 / 0.0223

Therefore, the molar mass of the unknown gas is 89.7 g/mol

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100g/mol

Explanation:

Given parameters:

Mass of unknown gas  = 2g

Volume of gas in flask  = 500mL  = 0.5dm³

Unknown:

Molar mass of gas = ?

Solution:

Since we know the gas is at STP;  

        1 mole of substance occupies 22.4dm³ of space at STP

    Therefore,

            0.5dm³ will have  0.02mole at STP

Now;

   Number of moles  =  

      Molar mass  =   =   = 100g/mol

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year