Answer:
The final volume is 990.8 L
Explanation:
Let calculate the moles of gas in the first situation:
P . V = n . R . T
1.20 atm . 2.90 L = n . 0.082 . 293K
(1.20 atm . 2.90 L) / (0.082 . 293K) = 0.145 moles
This are the same moles in the second situation:
P . V = n . R . T
0.003atm . V = 0.145 moles . 0.082 . 250K
V = (0.145 moles . 0.082 . 250K) / 0.003atm
V = 990.8 L
Answer: The final volume of the balloon is 990 L
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]
where,
[tex]P_1[/tex] = initial pressure of gas = 1.20 atm
[tex]P_2[/tex] = final pressure of gas = [tex]3.00\times 10^{-3}atm[/tex]
[tex]V_1[/tex] = initial volume of gas = 2.90 L
[tex]V_2[/tex] = final volume of gas = ?
[tex]T_1[/tex] = initial temperature of gas = [tex]20^oC=273+20=293K[/tex]
[tex]T_2[/tex] = final temperature of gas = [tex]-23^oC=273-23=250K[/tex]
Now put all the given values in the above equation, we get:
[tex]\frac{1.20\times 2.90}{293}=\frac{3.00\times 10^{-3}\times V_2}{250K}[/tex]
[tex]V_2=990L[/tex]
