A sample of a low-density gas is initially at room temperature and has pressure p0 . The gas is warmed at constant volume until the pressure is 2p0 .

Compared to the initial Celsius temperature of the gas, the final Celsius temperature is

A. greater by a factor of more than 2.

B. greater by a factor of 2.

C. greater by a factor between 1 and 2.

D. the same.

E. less

We can solve this problem by applying the pressure law, which states that for an ideal gas kept at constant volume, the ratio between the pressure and the absolute temperature of the gas is constant:

[tex]\frac{p}{T}=constant[/tex]

or

[tex]\frac{p_1}{T_1}=\frac{p_2}{T_2}[/tex]

where in this problem:

[tex]p_1 = p_0[/tex] is the initial pressure of the gas

[tex]T_1[/tex] is the initial absolute temperature (in Kelvin)

[tex]p_2 = 2 p_0[/tex] is the final pressure

[tex]T_2[/tex] is the final temperature in Kelvin

Re-arranging the equation,

[tex]\frac{p_0}{T_1}=\frac{2p_0}{T_2}\\T_2 = 2T_1[/tex]

So, the temperature in Kelvin has doubled. We can now rewrite this relationship by rewriting the Kelvin temperature in Celsius degrees:

[tex]T_{C2}-273 = 2(T_{C1}-273)\\T_{C2}=2T_{C1}-273[/tex]

where [tex]T_{C1}, T_{C2}[/tex] are the initial and final temperatures in Celsius degrees.

This means that the temperature in Celsius increases by a factor between 1 and 2, so the correct answer is C.

Learn more about ideal gases:

brainly.com/question/9321544

brainly.com/question/7316997

brainly.com/question/3658563

#LearnwithBrainly