The final temperature on increasing the pressure to 7.65 atm is 637 K.
Explanation:
The relation between temperature attained by gas molecules at varying pressure is defined by Guy-Lusac's law. It states that at constant volume, the pressure experienced by the gas molecules is directly proportional to the temperature attained by those molecules.
P∝T
Here, the initial pressure P₁ is given as 4 atm at temperature T₁ = 333 K, then the final pressure P₂ = 7.65 atm can be attained at temperature T₂.
The final temperature should be greater than the initial temperature as there is an increase in the pressure.
So,
[tex]\frac{P_{1} }{T_{1} } = \frac{P_{2} }{T_{2} }[/tex]
[tex]\frac{4}{333} =\frac{7.65}{T_{2} } \\\\T_{2} =\frac{7.65*333}{4} = 636.8 =637 K[/tex]
Hence, the final temperature on increasing the pressure to 7.65 atm is 637 K.
