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

========================

Answer 2

At STP (standard temperature and pressure), the volume of 1 mole of gas is 22.4 liters. Neon is a monoatomic gas, so 1 mole of neon contains 6.022 x 10^23 atoms. Therefore, the number of atoms of neon in 14.3 liters at STP can be calculated by proportion - (14.3/22.4) * 6.022 x 10^23.

Answer 3

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 4

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 5

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 6

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 7

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

Answer 8

0.638 moles

Answer 9

6.45