how would you find the empirical formula of a compound with %C=66.41, %H=5.58, %X=28.01 (where X is a halide)?
-
1] Choose, arbitrarily, a basis for calculation. I choose 100g
2] THat means there are 66.41 g C, 5.58 g H, and 28.01 g X
3] For C and H divide grams by atomic mass to get moles
4] That will give you CaHbXx
5] Now since you don't know what X [F, Cl, Br, I, At] is it is tougher....
6] So you could divide 28.01 by the atomic masses of each halogen [separately] and see if the x in Xx fits, that is, whether you can divide a, b, and x by some number to get an integer for all 3 after dividing.
2] THat means there are 66.41 g C, 5.58 g H, and 28.01 g X
3] For C and H divide grams by atomic mass to get moles
4] That will give you CaHbXx
5] Now since you don't know what X [F, Cl, Br, I, At] is it is tougher....
6] So you could divide 28.01 by the atomic masses of each halogen [separately] and see if the x in Xx fits, that is, whether you can divide a, b, and x by some number to get an integer for all 3 after dividing.