Question

A 3.50 L gas sample at 20.0 C and a pressure of 650. mm Hg is allowed to expand to a volume of 8.0 L. The final pressure of the gas is 425 mm Hg. What is the final temperature of the gas?

Answer 1

Answer:

437 K

Explanation:

initial PV/T = final PV/T

(3.50L)(650 mm Hg)/293K = (425 mm Hg)(8.0 L)/T2

7.78 T2 = 3,400

T2= 437 K

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Answer 2

The final temperature of the gas after the expansion has been 45.71$\rm ^\circ C$.

The final temperature of the gas can be calculated with the ideal gas equation. By value of constant has been equal at initial temperature and final temperature.

Initial $\rm \dfrac{PV}{T}$ = final $\rm \dfrac{PV}{T}$

P = pressure = 425 mm Hg

V = volume of gas

initial Volume = 3.5L

final volume = 8.0 L

T = temperature

Initial temperature = $\rm 20^\circ C$

Substituting the values;

$\rm \dfrac{425\;\times\;3.5}{20^\circC}\;=\;\dfrac{425\;\times\;8}{final\;temperature}$

Final temperature = 45.71 $\rm ^\circ C$.

Thus the final temperature of the gas after the expansion has been 45.71$\rm ^\circ C$.

For more information about the expansion of gases, refer to the link:

https://brainly.com/question/15304497