Question

Starting with a vessel of temperature 50.1°C, a pressure of 6263.MmHg and volume 461.1mL, what is its final volume, in liters, if you cool it to -95.8°C with a final pressure of 411.Atm?

Answer 1

Answer:

The value of final volume inside the vessel  $V_{2}$ =  5.17 ml

Explanation:

Initial pressure $P_{1}$ = 6263 mm Hg = 8.24 atm = 835 K pa

Initial temperature $T_{1}$ = 50.1 ° c = 323.1 K

Initial volume $V_{1}$ = 461.1 ml =  0.0004611 $m^{3}$

Final temperature $T_{2}$ = - 95.8 ° c = 177.2 K

Finial pressure $P_{2}$ = 411 atm = 41644.6 K PA

We know that

$P_{1} \frac{V_{1} }{T_{1} } = P_{2} \frac{V_{2} }{T_{2} }$

Put all the values in the above equation

⇒ 835 × $\frac{0.0004611}{323.1}$ = 41644.6 × $\frac{V_{2} }{177.2}$

⇒ $V_{2}$ = 5.07 × $10^{-6}$ $m^{3}$

⇒ $V_{2}$ =  5.17 ml

This is the value of final volume inside the vessel.