Answer :
Final answer:
Using Charles' Law, which states the volume and temperature of an ideal gas are directly proportional, we calculate that the temperature of the gas increases to 343.15°C when the volume is increased from 4.00 L to 8.00 L.
Explanation:
The principle at work here is Charles' Law, from the field of Physical Science, specifically Chemistry and Physics. Charles' law states that the volume and temperature of an ideal gas are directly proportional, provided the pressure and the amount of gas remain constant.
Given that, we first convert the initial Celsius temperature to Kelvin by adding 273.15, which gives us 308.15 K. Then, we can apply Charles' law as follows:
(V1 / T1) = (V2 / T2)
where V1 is the initial volume (4.00 L), T1 is the initial temperature (308.15 K), V2 is the final volume (8.00 L), and T2 is the final temperature, which we're trying to find.
Substituting and solving for T2 gives us:
T2 = (V2 * T1) / V1
So, T2 = (8.00 L * 308.15 K) / 4.00 L = 616.30 K
This is the final temperature of the gas in Kelvin. To convert this back to Celsius, subtract 273.15, which gives us 343.15°C.
Learn more about Charles' Law here:
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