A "neon" sign contains 2.4¡Ñ10^2mL of argon. Assuming that the gas is at standard temperature and pressure, there is 1.00 moles of gas per 22.4 L of volume. How many argon atoms are present in this sign?

use the convention; 22.4L = 1.00moles

so convert that volume of argon in neon sign to liters and fine the mole for that volume using the above convention.

then use this; 1 mole = 6.02e23 atoms to find the number of atoms in the mole you calculated above.

To find the number of argon atoms present in the sign, we can use the concept of Avogadro's number.

Step 1: Calculate the volume of the given argon gas in liters.
We are given that the sign contains 2.4 x 10^2 mL of argon. Since 1 liter is equal to 1000 mL, we can convert the volume to liters by dividing it by 1000:
2.4 x 10^2 mL ÷ 1000 = 0.24 L

Step 2: Calculate the number of moles of argon gas using the given volume.
According to the problem, there is 1.00 mole of gas per 22.4 L of volume. Using this relationship, we can find the moles of argon gas:
0.24 L × (1.00 mol/22.4 L) = 0.0107 mol

Step 3: Use Avogadro's number to calculate the number of argon atoms.
Avogadro's number states that there are 6.022 x 10^23 particles (atoms, molecules, or ions) in 1 mole of any substance. Therefore, to calculate the number of argon atoms present in the sign, we multiply the number of moles by Avogadro's number:
0.0107 mol × (6.022 x 10^23 atoms/1 mol) = 6.4534 x 10^21 argon atoms

Therefore, the sign contains approximately 6.4534 x 10^21 argon atoms.

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what is the answer?