49. (3pts) A student calculated the volume of a 2.71

mol sample of helium at 450 torr and 35 °C.

The student solved the problem using the ideal

gas law as shown below:

(450 torr) (V) = (2.71mol) (0.08206 Latm/mol) (35 °C)

What mistakes did he make in his set up?

Clearly list as many as you can identify.

The main errors seen in the formula are the pressure and temperature units. Units must be converted (from Torr to atm and from ° C to K). 760 Torr = 1 atm and 273K = 0 ° C

Explanation:

760 Torr---1 atm

450 Torr---x = (450 Torr x 1 atm) / 760 Torr = 0,59 atm

35 + 273 = 308K

PV = nRT (0,59atm) (V) = (2.71mol) (0.08206 Latm/mol) (308K)

V = ((2.71mol) (0.08206 Latm/mol) (308K)) / 0,59 atm = 116, 09 L