A "neon" sign contains 2.4¡Ñ102mL 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?
a. 6.5¡Ñ10^21
b. 2.8¡Ñ10^22
c. 3.2¡Ñ10^24
d. 9.9¡Ñ10^-23
I can't decipher the hieroglyphics in your post.
To find the number of argon atoms present in the neon sign, we need to follow these steps:
Step 1: Convert the given volume to liters.
2.4 x 10^2 mL = 2.4 x 10^-1 L (since 1 L = 1000 mL)
Step 2: Use the Avogadro's law to find the number of moles of argon.
According to Avogadro's law, 1 mole of any gas occupies 22.4 L at standard temperature and pressure (STP). So, the number of moles of argon can be calculated as:
n = V/Vm
n = 2.4 x 10^-1 L / 22.4 L/mole
n = 1.0714 x 10^-2 moles (rounded to four decimal places)
Step 3: Convert moles to atoms.
To convert moles to atoms, we use Avogadro's number, 6.022 x 10^23 atoms/mole.
The number of argon atoms can be calculated as:
Number of atoms = n x Avogadro's number
Number of atoms = 1.0714 x 10^-2 moles x 6.022 x 10^23 atoms/mole
Number of atoms = 6.4556 x 10^21 atoms (rounded to four decimal places)
Therefore, the number of argon atoms present in the neon sign is approximately 6.5 x 10^21.
So, the correct answer is:
a. 6.5 x 10^21