Respuesta :
Answer:
The molar mass of the gas is 43.5g/mol.
Explanation:
The given information of the gas from the exercise is:
- Volume (V): 250mL (0.25L)
- Mass: 0.435g
- Pressure (P): 743mmHg (1atm)
- Temperature (T): 29°C (302K)
1st) We can use the Ideal Gases formula to calculate the number of moles of the gas, remember to convert the units to atm, liters and Kelvin:
[tex]\begin{gathered} P*V=n*R*T \\ 1atm*0.25L=n*0.082\frac{atm*L}{mol*K}*302K \\ 0.25atm*L=n*25\frac{atm*L}{mol} \\ \frac{0.25atm*L}{25\frac{atm*L}{mol}}=n \\ 0.01mol=n \end{gathered}[/tex]2nd) Now we can calculate the molar mass of the gas using the mass and the 0.01 moles, with a mathematical rule of three:
[tex]\begin{gathered} 0.01mole-0.435g \\ 1mole-x=\frac{1mole*0.435g}{0.01mole} \\ x=43.5g \end{gathered}[/tex]Finally, the molar mass of the gas is 43.5g/mol.
