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

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

plz give brainliest

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.