A "neon" sign contains 2.4¡Ñ10^2 mL 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
Do you really expect an expert to answer all of your posted questions?
It's not going to happen! Jiskha tutors do not do homework for lazy students.
Ms Sue is right. I have given some information and/or hints to help working all of these except two or three. Those I will be happy to critique your work
To determine the number of argon atoms present in the sign, we need to first find the volume of the argon gas in liters, and then convert moles of argon to atoms.
Given:
- Volume of Argon gas (V) = 2.4 × 10^2 mL
- 1 mole of gas = 22.4 L
1. Convert the volume of argon gas from milliliters to liters:
Since 1 mL = 1 × 10^-3 L, we have:
V = 2.4 × 10^2 mL × 1 × 10^-3 L/mL
V = 0.24 L
2. Calculate the number of moles of the argon gas:
Given the molar volume at standard temperature and pressure of 22.4 L, we can use the formula:
Moles (n) = Volume (V) / Molar volume (V_molar)
n = 0.24 L / 22.4 L/mol
n = 0.0107 mol (rounded to four decimal places)
3. Convert moles to atoms:
To calculate the number of atoms, we will use Avogadro's number, which states that 1 mole of any substance contains 6.022 × 10^23 atoms.
Number of atoms = Moles (n) × Avogadro's number
Number of atoms = 0.0107 mol × 6.022 × 10^23 atoms/mol
Number of atoms ≈ 6.45 × 10^21 atoms
Therefore, the number of argon atoms present in the sign is approximately 6.5 × 10^21 (option a).