Question

A 7.2 mol sample of ammonia gas is in a 63.5 L container. What is the pressure of this gas at 350 oC?

Answer 1

The pressure of the gas is 5.8atm.

Step-by-step explanation:

The information given in the exercise is:

- Number of moles (n): 7.2mol

- Volume of the gas (V): 63.5L

- Temperature of the gas (T): 350°C (623K)

We can use the Ideal Gases formula to calculate the pressure of the gas, replacing the values of n, V and T.

Remember that the units must be always in atm, liters, mol and Kelvin when using the Ideal Gases formula:

`\begin{gathered} P*V=n*R*T \\ P*63.5L=7.2mol*0.082(atm*L)/(mol*K)*623K \\ P*63.5L=367.82atm*L \\ P=(367.82atm*L)/(63.5L) \\ P=5.8atm \end{gathered}`

So, the pressure of the gas is 5.8atm.