The number of moles in 9.63 L of H₂S gas :
[tex]\large{\boxed{\bold{0.4299}}[/tex]
Stochiometry in Chemistry studies about chemical reactions, especially on quantitative, such as the calculation of volume, mass, amount, which is related to the number of actions, molecules, elements, etc.
In chemical calculations the reactants can be determined, the amount of substances that can be expressed in units of mass, volume, moles or determine a chemical formula for example the levels of substances or hydrate molecular formulas.
Some of the laws regarding gas, can apply to ideal gas (volume expansion does not occur when the gas is heated), among others
So that the three laws can be combined into a single gas equation, the ideal gas equation
In general, the gas equation can be written
[tex] \large {\boxed {\bold {PV = nRT}}} [/tex]
where
P = pressure, atm
V = volume, liter
n = number of moles
R = gas constant = 0.082 L.atm / mole.K
T = temperature, Kelvin
The volume per mole of a gas is called the molar volume
[tex]\large {\boxed {\bold {V=n\times\: Vm}}[/tex]
V = volume of gas, liters
n = mole
Vm = molar volume (liters / mole)
Molar volume depends on conditions:
Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure).
If we input P = 1 atm and T = 0 C + 273 K
then the volume for every 1 mole of gas:
[tex]\displaystyle 1\:atm.V=1\:mole\times 0.082 \frac{L.atm}{mole.K}\times 273\:K[/tex]
[tex]\boxed{\bold{V=22.4\:L}}[/tex]
So, at STP, Vm is 22.4 liters / mole gas
Conditions at T 25 ° C and P 1 atm are stated by RTP (Room Temperature and Pressure). Vm in this condition = 24.4 liters / mol e
Given:
9.63 L of H₂S gas
The number of moles at STP :
[tex]\displaystyle mole=n=\frac{V}{Vm}\\\\n=\frac{9.63\:L}{22.4\:L}\\\\n=0.4299\:moles[/tex]
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Keywords: gas, STP, molar volume, H₂S
