Answer:
30.0g/mol
Explanation:
Step 1: Given data
Step 2: Calculate the moles of the gas
We will use the ideal gas equation.
[tex]P \times V = n \times R \times T\\n = \frac{P \times V}{R \times T} = \frac{1atm \times 0.0933L}{\frac{0.0821atm.L}{mol.K} \times 273.15K} = 4.16 \times 10^{-3} mol[/tex]
Step 3: Calculate the molar mass of the gas
4.16 × 10⁻³ moles correspond to a mass of 0.125 g. The molar mass of the gas is:
[tex]\frac{0.125g}{4.16 \times 10^{-3} mol} =30.0g/mol[/tex]
The molar mass of the 0.125 g of the gas occupies 93.3 mL at STP is 30.0 g/mol.
Number of moles of Gas at STP,
[tex]\bold{n =\dfrac {PV}{RT}}[/tex]
where,
P - pressure
V- volume
R- gas constant
T - temperature
Put the values in the formula,
[tex]\bold{n =\dfrac {1 \times 0.0933} {0.082 \times 273.15 }}\\\\\bold{n =4.16 \timesw 10^-^3}[/tex]
The molar mass of the gas can be calculated using formula,
[tex]\bold {m = \dfrac {w}{n}}\\\\\bold {m = \dfrac {0.125} {4.16 \times 10^-^3}}\\\\\bold {m = 30g/mol}[/tex]
The molar mass of the 0.125 g of the gas occupies 93.3 mL at STP is 30.0 g/mol.
To know more about molar mass, refer to the link:
https://brainly.com/question/12127540
