How many atoms of neon occupy a volume of 14.3 liters at STP?

Answer 1

Use the ideal gas equation.

PV = nRT

(1 atmosphere)(X volume) = (0.350 moles Ne)(0.08206 L*atm/mol*K)(298.15 K)

Volume = 8.56 Liters of neon gas

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Answer 2

As far as I understood and found in my chemistry book, the answer to this question is 0.638:

14.3 L X 1 mole / 22.4 L= 0.638

Answer 3

PV=nRT

P=1 ATM at STP

n is # of moles

R is ideal gas constant (here use, .0821 L*ATM/(mol * K)

T = 273 K at STP

V = volume

Plug and chug

Answer 4

Using 6.02x10^23 for Avogadros number, and 22.4 for the conversion factor at STP, there are 3.84x10^23 atoms of neon present.

Answer 5

Using the combined gas law of PV = nRT and substituting values...

(0.83 atm)(2.2 L) = n(0.0821Latm/degmole)(283deg)

n = (0.83)(2.2)/(0.0821)(283) = 0.0786 L = 0.079 liters

Answer 6

O.8 moles of 122.4 L of neon at STP.

Answer 7

0.638 moles

Answer 8

6.45