Question

What pressure (in atmospheres) is exerted by 0.400 moles of Xenon gas in a 3.18 L container at 260.0 K?2.312.472.202.69

Answer 1

Answer: the pressure exerted by this sample of gas is 2.69 atm

Step-by-step explanation:

The question requires us to calculate the pressure of a xenon gas, given that there are 0.400 moles of gas in a 3.18 L container at 260.0K.

We can apply the equation for ideal gases to solve this problem:

`PV=nRT`

where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of gas, T is the temperature and R is the constant of gases.

Since the question requires us to calculate the pressure in units of atmospheres (atm) and the volume of gas was given in litres, we can use the value of R as 0.082057 L.atm/K.mol.

First, let's rearrange the equation for ideal gases in order to calculate the pressure:

`PV=nRT\rightarrow P=(nRT)/(V)`

Next, applying the values given by the question, we'll have:

`\begin{gathered} P=((0.400mol)*(0.082057L.atm/K.mol)*(260.0K))/((3.18L)) \\ \\ P=2.69atm \end{gathered}`

Therefore, the pressure exerted by this sample of gas is 2.69 atm.