Question

If 3.0L of helium at 20°C is allowed to expand to 4.4L, with pressure remain the same.
What is the new temperature?​

Answer 1

Answer:

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Explanation:

We assume that the pressure and moles of helium gas remain constant and that it has ideal behavior. According to Charles's Law, the gas temperature and volume are proportional to each other, so we can write the following relation at two conditions, where the temperatures are in Kelvin:

V1T1=V2T2V1T1=V2T2

Initial volume (given) = V1=3.0 LV1=3.0 L

Initial temperature (given) = T1=20 oC+273.15=293.15 KT1=20 oC+273.15=293.15 K

Final volume (given) = V2=4.4 LV2=4.4 L

We solve for the final temperature using Charles's Law:

3.0 L293.15 K=4.4 LT2T2=430 K−273.15=157 oC