**On exams, you will be
expected
to calculate numerical answers, without being given certain basic
constants.**

You do not have to
memorize
this exact list, as long as the numbers you did memorize allow you to
do
equivalent calculations. For example, from a knowledge of
Avogadro's number and the chemical definition of a
mole, you can get the atomic mass unit in g (1 amu = 1.66 x 10^{-24}
g; this is just the reciprocal of Avogradro's number.)

k_{B} = 1.38 x 10^{-23}
J/K

N_{A}=6.02 x 10^{23}
molecules/mole

1 amu = 1.66 x 10^{-27}
kg

In addition to
fundamental
constants above, of course, you do have to memorize a few other
numbers.
The ones that come to mind are

g = 9.8 m/s^{2}

0^{o}C=273.15 K

1 atm = 10^{5}
Pa
(actually 1.013 x 10^{5} Pa, and 1 "Pascal" is 1 N/m^{2}.)

You probably have your
own
list of things you keep in your head, like 22.4 liters per mole at STP,
which would enable you to find how many pascals pressure is one
atmosphere
from the ideal gas formula, if you remember that "STP" is 0^{o}C
and 1 atm.

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