IN CASE YOU ARE NOT CONSIDERING:
During our review days I forget to point out that you need
to study the “mole road” please revise it.
mass  # mole  # particles
mass to # mole divide by MM & # mole to mass multiply by
MM
MM is molar mass & it is the sum of atomic masses
We get atomic mass from periodic table. The unit of MM is
g/mole. If it is an element its molar mass is the same as its
atomic mass. For diatomic elements (H,N,O,F,Cl,Br & I )
their molar mass is doble of their atomic mass (if they are
in their natural state).
# mole to # particle multiply by Avog.# &
#particle to # mole divide by Avog. #
Avog. # is 6,02*1023
The other important point is Limiting Reactants (LR) : If
the mass of two reactants is given do not forget first to
figure out the LR by comparing the # moles for the given
mass with the mole ratio from balanced equation, Once
you know the LR use that amount to find the theoretical
yield and other related question. (Please revise
stoichiometric calculations).
Also remember the Hf & Gf for elements in their natural
state is zero. Hf is Heat of formation.
GOOD LUCK