Answer:
The molar mass of the gas should be 43.0 g/mol.
Explanation:
1.Use the ideal gas law([tex]PV=nRT[/tex]) & the formula for moles and molar mass([tex]n=m/M[/tex]).
2.Insert the equation [tex]n=m/M[/tex] into [tex]PV=nRT[/tex] and re-arrange to solve for M(molar mass). [tex]M = mRT/PV[/tex]
3.Insert values and use the gas constant R = [tex]0.082 (L * atm)/(K * mol)[/tex] since the volume is in liters and the pressure is in atmosphere units.
[tex]M = mRT/PV = \frac{(1.98g)(0.082 L*atm/(K*mol))(305 K)}{(0.960 atm)(1.20 L)}[/tex]
4. Your answer should be 42.99 g/mol or 43.0 g/mol.
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