Answer:
619.2 K
Explanation:
We can solve this problem by using Charle's Law, which states that:
"For a fixed mass of an ideal gas kept at constant pressure, the volume of the gas is directly proportional to its absolute temperature"
Mathematically:
[tex]V\propto T[/tex]
where
V is the volume of the gas
T is the absolute temperature
The equation can be rewritten as follows for a gas that undergoes a transformation at constant pressure:
[tex]\frac{V_1}{T_1}=\frac{V_2}{T_2}[/tex]
where in this problem:
[tex]V_1=736 mL = 0.736 L[/tex] is the initial volume of the gas
[tex]T_1=15.0C+273=288 K[/tex] is the initial temperature
[tex]V_2=2.28 L[/tex] is the final volume of the gas
Solving for T2, we find the final temperature:
[tex]T_2=\frac{V_2 T_1}{V_1}=\frac{(2.28)(288)}{0.736}=892.2 K[/tex]
Converting into Celsius degrees,
[tex]T_2=892.2-273=619.2 K[/tex]
