- 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.

Answer : option c) heat is released during the process.explanation :

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.