Answer:
100.92 L
Explanation:
At STP,
Pressure = 1 atm
Temperature = 273.15 K
Given, moles = 4.50 moles
Volume = ?
Using ideal gas equation as:
[tex]PV=nRT[/tex]
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
1 atm × V = 4.50 moles × 0.0821 L.atm/K.mol × 273.15 K
⇒V = 100.92 L
100.8 L
Given:
n = 4.50 moles of nitrogen gas (N₂)
Question:
At STP, what is the volume of nitrogen gas?
The Process:
This is a simple stoichiometric calculation. We will find out the volume of gas measured at STP with the number of known moles.
Remember that at STP 1 mole of gas = 22.4 L or referred to as molar volume [tex]\boxed{ \ V_m \ }[/tex].
So, let us use the formula to calculate the N₂ gas volume at STP.
[tex]\boxed{ \ n = \frac{V}{V_m} \ } \rightarrow \boxed{ \ V = n \times V_m \ }[/tex]
[tex]\boxed{ \ V = 4.50 \ moles \times 22.4 \ L/mol \ }[/tex]
[tex]\boxed{\boxed{ \ V = 100.8 \ L \ }}[/tex]
Thus at STP, the volume of 4.50 moles of nitrogen gas equal to 100.8 L.
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Notes:
