Chemistry

Chemistry, 16.07.2019 08:30, rleiphart1

Acompound is 2.00% h by mass, 32.7% s by mass, and 65.3% o by mass. what is its empirical formula? the second step is to calculate the number of moles of each element present in the sample. to do this, you must divide the mass of each element by its molar mass. the masses of the elements present are: mass h = g mass s = g mass o = g

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Chemistry, 11.07.2019 09:50, 2xLaFlare

The last step is to calculate the percent by mass of each element in ammonium nitrate (nh4no3). the masses of the elements in one mole of the compound are: mass n = 28.0 g mass h = 4.0 g mass o = 48.0 g the molar mass of the compound is 80.0 g/mol. what is the mass of one mole of the compound?

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Chemistry, 02.08.2019 16:30, yasameenakbari

Acompound is 2.00% h by mass, 32.7% s by mass, and 65.3% o by mass. what is its empirical formula? the first step is to calculate the mass of each element in a 100-g sample of the compound. we use 100 g because it makes the calculations more straightforward. what is the mass of each element in a 100.0-g sample of the compound? mass h = g mass s = g mass o = g

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Chemistry, 26.08.2019 18:10, vdestiny858

Acompound is 2.00% h by mass, 32.7% s by mass, and 65.3%o by mass. what is its empirical formula? the first step is to calculate the mass of each element in a 100-g sample of the compound. we use 100 g because it makes the calculations more straightforward. what is the mass of each element in a 100.0-g sample of the compound? mass h = mass s = mass o = done

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Chemistry, 17.09.2019 05:30, courtneymccl

Which step would a student find the molecular formula of a compound from the empirical formula? multiply the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula. subtract the ratio of the actual mass of the compound to the empirical formula mass from the subscripts of the empirical formula. divide the ratio of the actual mass of the compound to the empirical formula mass by the subscripts of the empirical formula. add the ratio of the actual mass of the compound to the empirical formula mass to the subscripts of the empirical formula.

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Acompound is 2.00% h by mass, 32.7% s by mass, and 65.3% o by mass. what is its empirical formula?...

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