- If you have a balloon of gas at 0°C and 1 atm, how many gas particles do you have?
(Write the answer in both work and numeric form. For example, thirty three and 33)

22.4 L

Explanation:
The conditions for temperature and pressure provided to you actually correspond to the old definition of STP (Standard Pressure and Temperature).
Under these specific conditions,
1
mole of any ideal gas occupies
22.4 L
. This value is known as the molar volume of a gas.
You can show that this is the case by using the ideal gas law equation, which looks like this
P
V
=
n
R
T
−−−−−−−−−−
Here
P
is the pressure of the gas
V
is the volume it occupies
n
is the number of moles of gas present in the sample
R
is the universal gas constant, equal to
0.0821
atm L
mol K
T
is the absolute temperature of the gas
Rearrange the ideal gas law equation to
P
V
=
n
R
T
⇒
V
n
=
R
T
P
Plug in your values to find -- do not forget to convert the temperature from degrees Celsius to Kelvin
V
n
=
0.0821
atm
⋅
L
mol
⋅
K
⋅
(
273.15
+
0
)
K
1
atm
V
n
=
22.4 L mol
−
1
This means that under these conditions for pressure and temperature, you get
22.4 L
for every mole of an ideal gas present in a sample.
SIDE NOTE STP conditions are currently defined as a pressure of
100 kPa
and a temperature of
0
∘
C
.
Under these specific conditions, the molar volume of a gas is equal to
22.7 L mol
−
1
.

I HOPE THIS HELPS YOU AND I HOPE IS CORRECT AND IT WASN’t I’m sorry.