Answer:
The volume of the gas will be 78.31 L at 1.7 °C.
Explanation:
We can find the temperature of the gas by the ideal gas law equation:
[tex] PV = nRT [/tex]
Where:
n: is the number of moles
V: is the volume
T: is the temperature
R: is the gas constant = 0.082 L*atm/(K*mol)
From the initial we can find the number of moles:
[tex] n = \frac{P_{1}V_{1}}{RT_{1}} = \frac{1 atm*62.65 L}{(0.082 L*atm/K*mol)*(0 + 273)K} = 2.80 moles [/tex]
Now, we can find the temperature with the final conditions:
[tex] T_{2} = \frac{P_{2}V_{2}}{nR} = \frac{612.0 mmHg*\frac{1 atm}{760 mmHg}*78.31 L}{2.80 moles*0.082 L*atm/(K*mol)} = 274.7 K [/tex]
The temperature in Celsius is:
[tex] T_{2} = 274.7 - 273 = 1.7 ^{\circ} C [/tex]
Therefore, the volume of the gas will be 78.31 L at 1.7 °C.
I hope it helps you!
