Final answer:
To find the volume occupied by 10.3 g of neon at STP, first convert the mass to moles using the molar mass of neon and then multiply by the molar volume of a gas at STP (22.4 L/mol). The result is approximately 11.424 liters.
Step-by-step explanation:
The student is asked to determine the volume occupied by 10.3 g of neon gas at STP (Standard Temperature and Pressure). To solve this problem, we need to use the molar volume of a gas at STP, which is 22.4 liters per mole (L/mol).
First, we need to convert the mass of neon into moles by using the molar mass of neon, which is approximately 20.18 grams per mole (g/mol). We calculate the number of moles of neon as:
Number of moles = mass (g) ÷ molar mass (g/mol)
Number of moles = 10.3 g ÷ 20.18 g/mol
= 0.510 moles approximately
Next, using the molar volume of a gas at STP:
Volume at STP = moles × molar volume (L/mol)
Volume at STP = 0.510 moles × 22.4 L/mol
= 11.424 liters approximately
Therefore, 10.3 g of neon occupies approximately 11.424 liters at STP.