A given sample of xenon fluoride contains molecules of a single type, XeF_n, where n is some whole number. Given that 9.03 × 10²⁰ molecules of XeF_n weigh 0.311 g, calculate n.

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To find n, calculate the molar mass of XeF_n. First, find the number of moles: 9.03 × 10²⁰ molecules / 6.022 × 10²³ molecules/mol = 1.5 × 10^-3 mol. Then, calculate the molar mass: 0.311 g / 1.5 × 10^-3 mol = 207 g/mol. The molar mass of Xe is 131.3 g/mol, so the molar mass of F_n is 207 - 131.3 = 75.7 g/mol. Since each F atom is 19 g/mol, n = 75.7 / 19 ≈ 4.

A Given Sample of Xenon Fluoride Contains Molecules of a Single