Chemistry

Chemistry, 31.08.2019 03:40, aesthetickait

Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen.

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Chemistry, 21.07.2019 11:00, mia2286

Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen. determine the empirical formula for a compound that is 70.79 carbon, 8.91 hydrogen, 4.59 nitrogen, and 15.72 oxygen. c18h27no2 c18h27no3 c17h27no3 c17h26no3

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Chemistry, 05.10.2019 05:10, Bubba06

Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen. determine the empirical formula for a compound that is 70.79 carbon, 8.91 hydrogen, 4.59 nitrogen, and 15.72 oxygen. c17h27no3 c18h27no2 c18h27no3 c17h26no3

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Chemistry, 07.10.2019 18:00, BustD0wnAnt

A2.52 g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess o2 to yield 3.52 g of co2 and 0.839 g of h2o. another sample of the same compound, of mass 4.14 g, yielded 1.75 g of so3. a reaction to determine the nitrogen content was carried out on a third sample with a mass of 5.66 g and yielded 1.88 hno3 (assume that all of the nitrogen in hno3 came from the compound). calculate the empirical formula of the compound.express your answer as a chemical formula. enter the elements in the order: c, h, s, n, o.

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Chemistry, 07.10.2019 22:00, alayciaruffin076

To use combustion analysis data to determine an empirical formula a molecular formula expresses the number of each kind of atom in a molecule. for example, the molecular formula for propene, c3h6, indicates three carbon atoms and six hydrogen atoms per molecule. this also means that one mole of propene contains three moles of carbon and six moles of hydrogen. an empirical formula expresses the mole ratio of the elements. the empirical formula for propene is ch2, indicating twice as much hydrogen as carbon. when analyzing unknown compounds in a lab, it is often possible to identify the mole ratios, and thus the empirical formula, but not the molecular formula. notice that the molecular mass of propene, 3(12)+6(1)=42amu, is a multiple of the empirical formula mass, 1(12)+2(1)=14amu . an unknown compound contains only carbon, hydrogen, and oxygen (cxhyoz). combustion of 3.00 g of this compound produced 4.40 g of carbon dioxide and 1.80 g of water.how many moles of carbon, c, were in the original sample? how many moles of hydrogen, h, were in the original sample?

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