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How do you convert 4.00 moles of #N_2# to liters?

Answer 1

First we assume a temperature and pressure; the molar volume at #RT# and #1# #atm# is #25.4# #dm^3# #mol^-1#. We get a volume of slightly over #100# #L#.

Therefore, all that needs to be done is multiply the mole count by the molar volume:

#4*molxx25.4# #dm^3# #mol^-1# or #4*molxx25.4# #L# #mol^-1# (#1L=1*dm^3#) #=# #??" litres"#

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Answer 2

Jeremiah Adams

To convert moles to liters using the ideal gas law, you can use the formula:

( V = \frac{{n \times R \times T}}{{P}} )

Where:

( V ) = volume of gas (in liters)
( n ) = number of moles of gas
( R ) = ideal gas constant (0.0821 L atm / mol K)
( T ) = temperature (in Kelvin)
( P ) = pressure (in atm)

Assuming standard conditions (1 atm pressure and 273.15 K temperature), the equation simplifies to:

( V = \frac{{n \times 0.0821 \times 273.15}}{{1}} )

Plug in the value of ( n ) (4.00 moles of ( N_2 )):

( V = \frac{{4.00 \times 0.0821 \times 273.15}}{{1}} )

( V ≈ 89.6 , \text{liters} )

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.