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How many moles are in 4.3 x 1021 molecules of UF6?
To convert from molecules to moles, you divide the number of molecules by Avogadro's number (6.022 x 10^23). So, for 4.3 x 10^21 molecules of UF6, you would have approximately 0.0071 moles of UF6.
Calculate mass of uranium from 175.5 of uranium hexafluoride?
To calculate the mass of uranium, we need to know the molar mass of uranium hexafluoride (UF6), which is approximately 352 g/mol. Given that the sample has 175.5 g of UF6, we can calculate the mass of uranium by multiplying the molar mass of uranium by the ratio of the molar mass of uranium to the molar mass of UF6 (238.03 g/mol / 352 g/mol) and then multiplying by the mass of UF6 provided. This would result in approximately 119.196 g of uranium in 175.5 g of UF6.
How many moles are in 25 grams of UF6?
To calculate the number of moles in 25 grams of UF6, first determine the molar mass of UF6 (uranium hexafluoride) by adding the atomic mass of uranium (238.03 g/mol) to six times the atomic mass of fluorine (19.00 g/mol). This gives a molar mass of 238.03 + (6 * 19.00) = 352.03 g/mol. Next, divide the given mass of 25 grams by the molar mass to find the number of moles: 25 g / 352.03 g/mol ≈ 0.071 moles. Therefore, there are approximately 0.071 moles in 25 grams of UF6.
Reaction between UF6 H2O?
When uranium hexafluoride (UF6) reacts with water (H2O), it undergoes a violent exothermic chemical reaction that produces hydrogen fluoride (HF) gas and uranyl fluoride (UO2F2) as products. This reaction can release toxic fumes and should be handled with extreme caution due to the potential hazards associated with both UF6 and HF.
How do you find the empirical formula of a compound of uranium and fluorine that is composed of 67.6 percent uranium and 32.4 percent fluorine?
To find the empirical formula, divide the percentage composition of each element by its atomic masses to get the number of moles of each element. Then, divide both values by the smallest number of moles to get a whole number ratio. In this case, the ratio is approximately 1:3, so the empirical formula is UF3.
What compound is uf6?
UF6 is uranium hexafluoride, a chemical compound composed of one uranium atom and six fluorine atoms. It is a volatile, radioactive, and toxic compound commonly used in the production of nuclear fuel.
What is the reaction of U3O8 to UF6?
When U3O8 reacts with UF6, it forms UF4 (uranium tetrafluoride) and O2 (oxygen gas) as products. This reaction is a part of the conversion process to convert uranium oxide into a form suitable for enrichment in the nuclear fuel cycle.
Uranium hexafluoride uf6 is one of the densest gases known. what is its density at stp if 1 mole occupies 22.4 l report answer in grams per liter gl?
The molar mass of uranium hexafluoride (UF6) is 349.04 g/mol. At STP conditions (0°C and 1 atm), 1 mole of any gas occupies 22.4 L. Therefore, the density of UF6 at STP is (349.04 g/mol) / (22.4 L) ≈ 15.56 g/L.
What is a balanced chemical equation involving UF6?
The balanced chemical equation for the reaction of UF6 with water is: UF6 + 3H2O → UO2F2 + 4HF
What is a balanced chemical equation involving uranium hexafluoride?
The balanced chemical equation for the reaction of uranium hexafluoride with water is: UF6 + 3H2O → UO2F2 (uranyl fluoride) + 6HF
What is the chemical formula for one of the compounds of uranium?
An example: uranium hexafluoride, with the formula UF6.
Is fluorine used to make uranium?
Fluorine is used to prepare UF4, UF6, UO2F2.
