The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what is the final volume (mL) of the gas
$\begin{array}{lllc}
&P&V&T\\hline
\text { initial: } & 720~ {\mathrm{mmHg}} & 235 {\mathrm{~mL}} & 25^{\circ} \mathrm{C} \
\text { final: } & 860~ \mathrm{mmHg} & ? & 15^{\circ} \mathrm{C}
\end{array}$

A) 170. mL
B) 180. mL
C) 190. mL
D) 210. mL
E) None of the above

Question

The following data describes an initial and final state for an ideal gas. Given that the amount of gas does not change in the process, what is the final volume (mL) of the gas 
$\begin{array}{lllc}
&P&V&T\\hline
\text { initial: } & 720~ {\mathrm{mmHg}} & 235 {\mathrm{~mL}} & 25^{\circ} \mathrm{C} \
\text { final: } & 860~ \mathrm{mmHg} & ? & 15^{\circ} \mathrm{C}
\end{array}$

A) 170. mL
B) 180. mL
C) 190. mL
D) 210. mL
E) None of the above

Quizplus · Accepted Answer

We can use the combined gas law to solve for the final volume:

(P1V1)/(T1) = (P2V2)/(T2)

Here are the known values:

P1 = 1.00 atm
V1 = 200. mL
T1 = 300. K
P2 = 0.600 atm
V2 = ?
T2 = 273. K

Solving for V2, we get:

V2 = (P1V1T2)/(P2T1)
V2 = (1.00 atm)(200. mL)(273. K)/((0.600 atm)(300. K))
V2 = 190. mL

Therefore, the final volume of the gas is 190. mL.

The Following Data Describes an Initial and Final State for an Ideal