Question

A student has a sample of 1.24 moles of fluorine gas that is contained in a 21.5 L container at 284 K. What is the pressure of the sample? The ideal gas constant is 0.0821 L*atm/mol*K. Round your answer to the nearest 0.01 and include units.

Answer 1

The pressure of the sample is 1.18atm.

Step-by-step explanation:

1st) The given information from the exercise is:

- Number of moles (n): 1.24moles

- Volume (V): 24.5L

- Temperature (T): 284K

- Ideal gas constant: 0.0821 atm*L/mol*K

2nd) With the Ideal Gases formula, we can replace the values of n, V and T to calculate the pressure of the sample:

`\begin{gathered} P*V=n*R*T \\ P*24.5L=1.24mol*0.0821(atm*L)/(mol*K)*284K \\ P*24.5L=28.91atm*L \\ P=(28.91atm*L)/(24.5L) \\ P=1.18atm \end{gathered}`

So, the pressure of the sample is 1.18atm.