Answer: 0.0812 atm
Explanation: The final pressure [tex](P_2)[/tex] can be found using the combined gas law [tex]\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}[/tex], where [tex]P_1[/tex] is 0.140 atm, [tex]V_1[/tex] is 2.00L, [tex]T_1[/tex] is [tex](-20^oC+273=253K)[/tex], [tex]V_2[/tex] is 4.50L, and [tex]T_2 = (57.0^oC + 273K = 330K)[/tex]. By plugging in all these values into the combined gas law equation: [tex](\frac{(0.140)(2.00)}{(253)} = \frac{(P_2)(4.50)}{(330)} )[/tex], [tex]P_2[/tex] is found to be 0.08115942 atm, which can be rounded to 0.812 atm with 3 significant figures.
