The volume of a gas with an initial pressure of 350 mmhg increases from 5.0 l to 8.0 l. what is the final pressure of the gas, in atm, assuming no change in moles or temperature? g

Use the ideal gas law for this problemP1V1 = n1RT1 (1)P2V2 = n2RT2 (2) Dividing equation (2) by equation (1), and note that n1 = n2, T1 = T2, you have the familiar Boyle's Law:
P1V1 = P2 V2whereP1 = 350 mmHgV1 = 5.0 LV2 = 8.0 L
350 (5) = P2(8)1750/8 = P2218.75 mmHg = P2
Divide the answer to 760.0 mm Hg because that represents 1 atm
So the final pressure P2 is 760 mmHg or 0.29 atm.

Atomicity occurs to prevent updates of the database occurring only partially, which can cause greater problems than rejecting the whole series outright.some are monatomic, diatomic, triatomic etc because it shows the number of atoms. for example, monatomic means it contains only one atom.