Molar
Mass
Mass
The molar mass of Boron. (Rounded to the nearest hundredth)
What is . . .
10.81 g
The number of particles in one mole.
What is . . .
6.02 x 1023 particles
To change from the mass of a substance to the number of particles you should do these two general steps.
What is . . .
1 divide by the molar mass
2. multiply by 6.02 x 1023
True or false: The empirical formula shows the lowest ratio of the elements in a compound.
What is . . .
True
True or false: A molecular formula shows the ratio of elements that actually exist.
What is . . .
True
The molar mass of CO2
What is . . .
44.01 g
The mass of 2 moles of beryllium (Be)
What is . . .
18.02 g
The number of atoms in 24.02 g of Carbon.
What is . . .
1.2 x 1024 atoms
Of the following, this formula would represent an empirical formula:
C3H6O3
C6H12O6
CH2O
CH2O
Of the following, which would be a molecular formula based on the empirical formula HO :
H2O NaOH H2O2
What is . . .
H2O2
The molar mass of Aluminum oxide: Al2O3
What is . . .
101.96 g
The number of moles in 101.02 g of Sulfur
What is . . .
about 3.15 moles
The mass of
2.2 x 1024 atoms of iron (Fe).
What is . . .
204 g
When calculating the empirical formula, a student determines that the substance has a ratio of
2.02 moles Chlorine,
2.02 moles Carbon, and
4.04 moles hydrogen.
This would be how they would write the empirical formula.
What is . . .
ClCH2
(Count as correct if anyone changed the order of elements if subscripts are correct.)
This would be the molecular formula for a compound with a molar mass of 88.12g/mol and an empirical formula of C2H4O
What is . . .
C4H8O2
The molar mass of Mg(NO3)2
What is . . .
148.33 g
The number of moles in
2.35 x 1024 atoms of sodium
What is . . .
3.9 moles
The mass of
3.6 x 1023 particles of H2O.
What is . . .
10.77 g
This is the empirical formula of a substance that is composed of 1.11g Se and 1.61g F.
What is . . .
SeF6
This would be the molecular formula for a compound that has an empirical formula of P2O5 and a molar mass of 283.88g
What is . . .
P4O10
The molar mass of calcium hydroxide.
What is . . .
74.1 g
for Ca(OH)2
The mass of 7.8 moles of H2O2
What is . . .
265.356 g
(Ok if rounded sooner.)
The mass of 8.7 x 1022 particles of Al2O3
What is . . .
14.74 g
The empirical formula for a substance that is made of 48.6% carbon, 8.16% hydrogen, and 43.2 % oxygen.
What is . . .
C3H6O2
Take your time on this: A compound contains only nitrogen and oxygen is 30.4% nitrogen by mass and 69.6% oxygen by mass. This is the molecular formula of the compound if the molar mass is 92 g/mol. Hint: First determine the empirical formula and then find the molecular formula.
What is . . .
N2O4