Question

0.6500 moles of H₂(g) are injected into a previously evacuated 1.00 L flask. The pressure is determined tobe 15.0 atm. What is the temperature of the gas under these conditions (in "C)?

Answer 1

The temperature of the gas is 8.28 °C.

Step-by-step explanation:

The given information from the exercise is:

- Number of moles (n): 0.6500 moles

- Volume (V): 1.00L

- Pressure (P): 15.0atm

With the Ideal Gases Law formula, we can calculate the temperature of the gas, by replacing the values of n, V and P:

`\begin{gathered} P*V=n*R*T \\ 15.0atm*1.00L=0.6500mol*0.082(atm*L)/(mol*K)*T \\ 15.0atm*L=0.0533(atm*L)/(K)*T \\ (15.0atm*L)/(0.0533(atm*L)/(K))=T \\ 281.43K=T \end{gathered}`

Finally, we have to convert 281.43K to °C:

281.43 - 273.15 = 8.28°C

So, the temperature of the gas is 8.28 °C.