Question

How many atoms of neon gas are there in 90.0L Ne at 0 degrees C and 1 atm of pressure? Make sure to round to the correct number of sig figs and include the unit in your final answer.

Answer 1

To determine the number of atoms in 90.0L Ne at standard conditions (0 °C, 1 atm), we find the number of moles by dividing the volume by the volume of 1 mole at STP, then multiply by Avogadro's number. The calculation results in approximately 2.42 x 10²´ atoms of neon.

Step-by-step explanation:

To calculate the number of atoms of neon gas in 90.0 L at 0 degrees C and 1 atm of pressure, we use the ideal gas law where the volume of 1 mol of an ideal gas is 22.41 L at 0 °C and 1 atm. First, we find the number of moles of Ne in 90.0 L:

Number of moles = (Volume of gas in L) / (Volume of 1 mole at STP in L) = 90.0 L / 22.41 L/mol

Then, we use Avogadro's number, which is 6.022 x 10²³ atoms/mol, to find the total number of atoms:

Number of atoms = Number of moles x Avogadro's number

Let's calculate:

1. Number of moles of Ne in 90.0 L = 90.0 L / 22.41 L/mol = 4.015 moles (rounded to 4 significant figures to match the volume given)
2. Number of atoms of Ne = 4.015 moles x 6.022 x 10²³ atoms/mol = 2.417 x 10²´ atoms

Therefore, there are approximately 2.42 x 10²´ atoms of neon gas in 90.0L Ne at 0 degrees C and 1 atm of pressure, rounded to three significant figures.