Question

At 1.344 atm and 51.8 °C a sample of gas occupies 288.5 L. What volume does it occupy at 0.324 atm and 7.6 °C?a. 1030O b. 176O c. 49.3Od. 1.03e8Check

Answer 1

The volume is 1,194 L. (The closest option is 1030L).

Step-by-step explanation:

The given information from the exercise is:

- Initial pressure (P1): 1.344atm

- Initial temperature (T1): 51.8°C (324.8K)

- Initial volume (V1): 288.5L

- Final pressure (P2): 0.324atm

- Final temperature (T2): 7.6°C (280.6K)

1st) We can solve this exercise using the Ideas Gases Formula, but first it is important to convert the temperature unit from °C to Kelvin:

- T1 conversion:

`51.8+273=324.8K`

-T2 conversion:

`7.6+273=280.6K`

2nd) Now we can replace the values of P1, T1, V1, P2 and T2 in the following formula, to calculate the final volume (V2):

`\begin{gathered} (P_1*V_1)/(T_1)=(P_2*V_2)/(T_2) \\ (1.344atm*288.5L)/(324.8K)=(0.324atm*V_2)/(280.6K) \\ 1.194(atm*L)/(K)=0.001(atm)/(K)*V_2 \\ (1.194(atm*L)/(K))/(0.001(atm)/(K))=V_2 \\ 1,194L=V_2 \end{gathered}`

So, the volume is 1,194 L. (The closest option is 1030L).