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A 0.395 g sample of a compound containing only chromium , sulfate and water of hydration, after heating to drive off the water of hydration, weights 0.213 g . A second sample weighting 0.706 g is dissolved in water and excess aqueous barium chloride is added to precipitate 0.601 g of barium sulfate . Calculate the empirical formula of the compound. Use asterisk * to specify molecular water of hydration.
How many moles of UF6 would have to be decomposed to provide enough fluorine to prepare 1.25 mol of CF4? ( Assume sufficient carbon is available.)
Why are moles used when all stoichiometry problems could be done using only the mass in grams of an atomic mass unit?
How many moles of UF6 would have to be decomposed to provide enough fluorine to prepare 1.25 mol of CF4? ( Assume sufficient carbon is available.)
Why are moles used when all stoichiometry problems could be done using only the mass in grams of an atomic mass unit?