What is the molecular formula of a substance that decomposes into 1.33 g of h and 21.3 g of o, and was found to have a molar mass of 34.1 g?

H2O2 First, let's determine how many moles of hydrogen and oxygen atoms we have. Start by looking up the atomic weights of those elements: Atomic weight hydrogen = 1.00794 Atomic weight oxygen = 15.999 Moles hydrogen = 1.33 g / 1.00794 g/mol = 1.319522987 mol Moles oxygen = 21.3 g / 15.999 g/mol = 1.331333208 mol We now have a ratio of 1.319522987 : 1.331333208 and we want a ratio of small integers that is close. Start by dividing all the numbers in the ratio by the smallest value, giving: 1 : 1.008950371 This ratio is acceptably close to 1:1 so I assume the formula is of the form HnOn where n is a small integer. Let's initially assume that n is 1, so the mass would be 1.00794 + 15.999 = 17.00694 Obviously 17 is far smaller than 34.1. So let's divide 34.1 by 17.00694 and see what n should be: 34.1 / 17.00694 = 2.005063815 So the formula we want is H2O2, which is hydrogen peroxide.

Outermost (valence) electrons

What record? the question is incomplete