When 5.095 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 15.61 grams of CO₂ and 7.457 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula = Previous Next

Q: A sample contains 43.7% phosphorus and 56.3% oxygen by mass. Determine its empirical formula. Write…

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Q: O hydrogen peroxide O tetraphosphorus decoxide O disilicon hexachloride O ammonia

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Q: Analysis of a white solid showed that it contained 22.56% phosphorus and some amount of chlorine.…

A: Empirical formula of the given compound is PCl3.

Q: Sample When 3.596 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus,…

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Q: Example How many molecules of O, are present in 6.25 moles? (why is this a molecule and not an…

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Q: what is the empirical formula of vanillin

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Q: 2. The analysis of 1.00 g sample of phosphorus oxide, with a molar mass of about 284 g/mol, was…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.