Question

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.

Answer 1

Answer:

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