The volume of a gas is 5.345 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume is changed to 9.65 L while the temperature remains constant?

Answer 1

Constant temperature is an example of Boyle's law:

P1V1 = P2V2

P1 = initial pressure = 1.00 atm

V1 = initial volume in L = 5.345 L

P2 = final pressure in atm = ?

V2 = final volume in L = 9.65

Substitue an solve for P2:

(1.00 atm)(5.345 L) = (P2)(9.65 L)

P2 = 0.553 atm

But the question asks for the pressure in mm Hg. The conversion of atm to mm Hg is as follows:

0.553 atm x 760 mm Hg / 1 atm = 421 mm Hg (3 sig. figs.)