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
I can't decipher the hieroglyphics.
what's the ¡Ñ???..unless it don't matter, then just convert the mL to liters such that;
240mL becomes 0.24L.
using the convention 1mole = 22.4L, find the mole for the 0.24L.
i.e. 0.24L/22.4 = 1.07e-2moles.
using avogadros number;
1mole = 6.02e23 atoms
i.e. 1.07e-2moles x 6.02e23 = 0.0645e23 atoms
unless the ¡Ñ matters to the unit, then you have to recheck the conversion and follow the same method above...
hope that helps...
To find the number of argon atoms present in the sign, we need to use the concept of Avogadro's number and the molar volume of a gas at standard temperature and pressure.
1 mole of any gas contains 6.022 x 10^23 atoms or molecules, which is known as Avogadro's number. And at standard temperature and pressure (STP), the molar volume of a gas is 22.4 liters.
Given that the volume of the argon gas in the sign is 2.4 x 10^2 mL, we need to convert it to liters by dividing it by 1000 since there are 1000 milliliters in a liter.
Volume of Argon gas = 2.4 x 10^2 mL = (2.4 x 10^2 mL) / (1000 mL/L) = 0.24 L
Now, we can calculate the number of moles of argon gas using the given molar volume:
Moles of Argon gas = Volume of Argon gas / Molar volume = 0.24 L / 22.4 L/mol = 0.0107 moles
Since 1 mole of any gas contains 6.022 x 10^23 atoms, the number of argon atoms present can be calculated by multiplying the number of moles by Avogadro's number:
Number of argon atoms = Moles of Argon gas x Avogadro's number = 0.0107 moles x 6.022 x 10^23 atoms/mole
Calculating the above expression, we get:
Number of argon atoms = 6.456 x 10^21
So, the correct answer is (a) 6.5 x 10^21 argon atoms.