after substantial heating, 0.194g of uranium produced 0.233g of a compound with oxygen. the empirical formula
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An oxide of uranium contains 84.8% of uranium. The empirical formula of the oxide is ? ( atomic mass of U = 238 , O = 16)
Sima S.
The mineral uraninite is a uranium oxide that is $84.80 \%$ uranium by mass. Show calculations to determine the correct empirical formula of uraninite.
A Uranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. This question considers some uranium chemistry. (a) $\mathrm{A}$ small sample of uranium metal $(0.169 \mathrm{g})$ is heated to between 800 and $900^{\circ} \mathrm{C}$ in air to give $0.199 \mathrm{g}$ of a dark green oxide, $\mathrm{U}_{x} \mathrm{O}_{y} .$ How many moles of uranium metal were used? What is the empirical formula of the oxide, $\mathrm{U}_{x} \mathrm{O}_{y} ?$ What is the name of the oxide? How many moles of $\mathrm{U}_{x} \mathrm{O}_{y}$ must have been obtained? (b) The naturally occurring isotopes of uranium are $^{234} \mathrm{U},^{235} \mathrm{U},$ and $^{238} \mathrm{U} .$ Knowing that uranium's atomic weight is $238.02 \mathrm{g} / \mathrm{mol},$ which isotope must be the most abundant? (c) If the hydrated compound $\mathrm{UO}_{2}\left(\mathrm{NO}_{3}\right)_{2} \cdot z \mathrm{H}_{2} \mathrm{O}$ is heated gently, the water of hydration is lost. If you have $0.865 \mathrm{g}$ of the hydrated compound and obtain $0.679 \mathrm{g}$ of $\mathrm{UO}_{2}\left(\mathrm{NO}_{3}\right)_{2}$ on heating, how many waters of hydration are in each formula unit of the original compound? (The oxide $\mathrm{U}_{x} \mathrm{O}_{y}$ is obtained if the hydrate is heated to temperatures over $800^{\circ} \mathrm{C}$ in the air.)
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