Question

30.0g of C2H6 gas are held in a container at 960 mmHg, at 275K. Determine thevolume of this container in mL.

Answer 1

The volume is 18,000mL.

Step-by-step explanation:

The given information from the exercise is:

- C2H6 gas

- Mass: 30.0g

- Pressure: 960mmHg

- Temperature: 275K

1st) To calculate the volume it is necessary to use the Ideal Gas formula, making sure that the variables are in atm, liters, mole and Kelvin.

- Conversion of 960mmHg to atm:

`960mmHg*(1atm)/(760mmHg)=1.26atm`

- Conversion of 30.0g to moles, using the molar mass of C2H6 (30g/mol):

`30.0g*(1mole)/(30g)=1mole`

The number of mole is 1.

2nd) Now we can replace the values in the Ideal Gas formula to find the volume:

`\begin{gathered} P*V=n*R*T \\ 1.26atm*V=1mol*0.082(atm*L)/(mol*K)*275K \\ 1.26atm*V=22.55atm*L \\ V=(22.55atm*L)/(1.26atm) \\ V=18.0L \end{gathered}`

3rd) Finally, we have to convert the liters to mL:

`18.0L*(1000mL)/(1L)=18,000ml`

So, the volume is 18,000mL.