Question

A syringe containing 35.0mL of axe gas at 298 K has a pressure of 0.980 atm. How many grams of ace are in the syringe?report you answer to the nearest 0.001 g.

Answer 1

There are 0.186g of Xe.

Step-by-step explanation:

The information given in the exercise is:

- Volume: 35.0 mL (0.035L)

- Temperature: 298 K

- Pressure: 0.980 atm

1st) We can calculate the moles of the gas with the Ideal Gases formula, by replacing the values of volume, temperature and pressure.

Remember that the variables units must be atm, L, mol and Kelvin when using the Ideal Gases formula:

`\begin{gathered} P*V=n*R*T \\ 0.980atm*0.035L=n*0.082(atm*L)/(mol*K)*298K \\ 0.0343atm*L=n*24.4(atm*L)/(mol) \\ (0.0343atm*L)/(24.4(atm*L)/(mol))=n \\ 1.41*10^(-3)moles=n \end{gathered}`

Now we know that there are 1.41x10^-3 moles of gas.

2nd) Finally, we have to convert the moles to grams, using the molar mass of Xe (132g/mol):

`1.41*10^(-3)moles*(132g)/(1mol)=0.186g`

So, there are 0.186g of Xe.