Astudent collects 350 ml of a vapor at a temperature of 67°c. the atmospheric pressure at the time of collection is 0.900 atm. how many moles of the gas does the student collect?

0.011 moles.
0.053 moles
0.11 moles
0.53 moles

First option 0.011 moles

Explanation:

You need to use the formula for Ideal gases which is:

PV = nRT

Where:

P = Pressure (in atm)

V = Volume (In Liters)

n = moles

R = gas constant (this depends of the units; in this case is 0.082 L atm/K)

T = temperature (In K)

From the formula above, we can solve for n:

n = PV / RT

Let's convert first the temperature and volume to K and L respectively:

T = 67 + 273 = 340 K

V = 350 mL / 1000 = 0.35 L

Finally, let's put all the values in the formula above to solve for the value of n:

n = 0.9 * 0.35 / 0.082 * 340

n = 0.315 / 27.88

n = 0.011 moles

0.88m hope i am correct : )

answer: atomic mass was originally used to arrange elements on the periodic table, but is no longer used to organize the modern version.

explanation:

originally atomic mass was used to arrange elements on the periodic table from left to right in a row. each column then shows similar properties of elements of a group.

in modern periodic table, the atoms are arranged in increasing atomic number. as atomic number represents the number of protons in an atom which is unique for every atom.