Achemist prepares a sample of helium gas at a certain pressure, temperature and volume and then removes all but a fourth of the gas molecules (only a fourth remain). how must the temperature be changed (as a multiple of t1) to keep the pressure and the volume the same? a. t2=1/16t1b. t2=2t1c. t2=16t1d. t2= 1/2t1e. t2=4t1f. none of theseg. t2=1/4t1

e. T₂= 4T₁

Explanation:

Initially, we have a number of moles (n₁) a gas sample at a certain pressure (P), temperature (T₁) and volume (V). We can relate these variables through the ideal gas equation.

P . V = n₁ . R . T₁

where,

R is the ideal gas constant

We can rearrange this equation like:

If only one fourth of the initial molecules remain n₂ = 1/4 n₁. The new temperature (T₂) assuming pressure and temperature remain constant is:

lol for the pointsss