a container of gas has a pressure of 1.45 atm at a temperature of 52 degrees celsius, if the pressure increases to 4.2 atm what would be the final temperature of the volume is held constant?

941 K (668°C)

Explanation:

We have the following data:

Initial pressure : P1 = 1.45 atm

Initial temperature: T1 = 52°C + 273 = 325 K

Final pressure: P2 = 4.2 atm

Final temperature: T2 = ?

The relation between pressure and temperature for a gas at constant volume is given by Gay-Lussac's law:

P1/T1 = P2/T2

That means that the pressure is directly proportional to the absolute temperature (in K). So, we calculate T2 from the equation:

T2 = P2 x T1/P1 = 4.2 atm x (325 K/1.45 atm) = 941 K

Therefore, the final temperature would be 941 K (668°C). This is consistent with the law, that states that if the pressure increase, the temperature will be increased.  

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