Question

30 points

You have a 7.00-liter container with 1.88 x10^23 molecules of methane gas, CH4, at STP. How many molecules of nitrogen gas, N2, are in an identical container at the same temperature and pressure?


2.00 x1023

2.00 x1024

1.88 x1023

1.80 x1024

EDIT: the answer is 1.88 x1023

Answer 1

1.88x10²³

Step-by-step explanation:

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Answer 2

1.88x10²³ molecules of N₂

Step-by-step explanation:

If the N₂ is at STP conditions and occupies 7L of volume, like the CH₄ we can apply the Ideal Gases Law to find out the moles.

STP = 273K (temperature) and 1atm (pressure)

P .V = n .R.T

1atm . 7L = n . 0.082L.atm/mol.K . 273K

(1atm . 7L) / (0.082L.atm/mol.K . 273K) = n

0.312 moles = n

These are the moles of N₂, so how many molecules are on it?

1 mol has NA molecules

0.312 moles have ____ ( 0.312 .NA) = 1.88x10²³

NA = Avogadro's number (6.02x10²³)