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

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

a corroding iron, if that's one of your choices