Answer:
5.58*10⁻³ moles of gas are in the sample.
Explanation:
The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.
Being 1000 mL equivalent to 1 L, then 125 mL is equal to 0.125 L. Then you can apply the following rule of three: if by STP conditions 22.4 L are occupied by 1 mole, 0.125 L are occupied by how many moles?
[tex]amount of moles=\frac{0.125 L*1 mole}{22.4 L}[/tex]
aomunt of moles= 5.58*10⁻³ moles
5.58*10⁻³ moles of gas are in the sample.
Answer:
5.58×10⁻³ moles of gas
Explanation:
There is a rule that says, that 1 mol of any gas, at STP is contained at 22.4L of volume.
We can apply a conversion factor
0.125 L . 1 mol / 22.4 L = 5.58×10⁻³ moles
Notice we converted volume from mL to L
We can also aply the Ideal Gases Law.
At STP we have 1 atm of pressure and 273.15K of T°
We replace data: 0.125 L . 1 atm = n . 0.082 . 273.15K
(0.125 L . 1 atm) / (0.082 . 273.15 K) = n
n = 5.58×10⁻³ moles
