Answer: The final volume is 1108 ml
Explanation:
According to combined gas law:
[tex]\frac{P_1V_1}{n_1T_1}=\frac{P_2V_2}{n_2T_2}[/tex]
Where :
[tex]P_1[/tex] = initial pressure = 1.000 atm
[tex]V_1[/tex] = initial volume = 550.0 ml
[tex]n_1[/tex]= initial moles = 4.50
[tex]T_1[/tex] = initial temperature = [tex]5.000^0C=(273+5.000)=278.00K[/tex]
[tex]P_2[/tex] = final pressure = 1.250 atm
[tex]V_2[/tex] = final volume = ?
[tex]n_2[/tex]= final moles = 10.50
[tex]T_2[/tex] = final temperature = [tex]27.00^0C=(273+27.00)K=300.0K[/tex]
[tex]\frac{1.000\times 550.0}{4.50\times 278.00K}=\frac{1.250\times V_2}{10.50\times 300.0}[/tex]
[tex]V_2=1108ml[/tex]
Thus final volume is 1108 ml
