The final temperature, in degrees Celsius, of the gas is 34.62 °C
From the question, we are to determine the final temperature, in degrees Celsius
From the Pressure law or Gay-Lussac's law
We have that, for a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature.
Using the formula,
[tex]\frac{P_{1} }{T_{1}} = \frac{P_{2} }{T_{2}}[/tex]
Where P₁ is the initial pressure
T₁ is the initial temperature
P₂ is the final pressure
and T₂ is the final temperature
From the given information,
P₁ = 739 mmHg
T₁ = 23 °C = 23 + 273.15 = 296.15 K
P₂ = 768 mmHg
T₂ = ?
Putting the parameters into the formula, we get
[tex]\frac{739}{296.15}=\frac{768}{T_{2} }[/tex]
Then,
[tex]T_{2} = \frac{768 \times 296.15}{739}[/tex]
T₂ = 307.77 K
Therefore,
T₂ = 307.77 - 273.15 = 34.62 °C
Hence, the final temperature, in degrees Celsius, of the gas is 34.62 °C
Learn more on Gas laws here: https://brainly.com/question/16478170
Here is the complete question:
A gas sample has a pressure of 739 mmHg when the temperature is 23 °C. What is the final temperature, in degrees Celsius, when the pressure is 768 mmHg, with no change in the volume or amount of gas?
