Question

At stp, what is the volume of 4.50 moles of nitrogen gas

Answer 1

100.8 L

Further explanation

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 $\boxed{ \ V_m \ }$.

So, let us use the formula to calculate the N₂ gas volume at STP.

$\boxed{ \ n = \frac{V}{V_m} \ } \rightarrow \boxed{ \ V = n \times V_m \ }$

$\boxed{ \ V = 4.50 \ moles \times 22.4 \ L/mol \ }$

$\boxed{\boxed{ \ V = 100.8 \ L \ }}$

Thus at STP, the volume of 4.50 moles of nitrogen gas equal to 100.8 L.

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Notes:

• STP (in chemistry) is the abbreviation for Standard Temperature and Pressure, i.e., 273 K (0° Celsius or 32° Fahrenheit) and 1 atm.
• Remember that the mole number of a substance can be found via mass, volume, or number of particles.

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Answer 2

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:

$PV=nRT$

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