9 posts • Page 1 of 1
After finding the molar ratio, would it be inaccurate to express the atom ratio in the same whole numbers as the molar ratio? My thought process would be as if the atoms cancel out if put in a ratio and only the whole numbers from the molar ratio would remain.
I would think that the molar ratio and the atom ratio are the same, so I do not think that it would be inaccurate. But when creating the molecular or empirical formula, you must have whole numbers denoting the number of atoms in a specific molecule.
If by molar ratio you're talking about the whole numbers that you get once you've manipulated the number of moles of each substance into a ratio (dividing by the smallest amount then multiplying all of those ratios by a scalar until they're all whole numbers), then yes, they are the same as the atom ratio (which is the empirical formula).
I answered with both the ratio I got by converting the percents to grams, then dividing by the g/mol to get the moles of each, then dividing each value by the lowest mole value (1.972), as well as a ratio in full numbers (empirical formula).
Who is online
Users browsing this forum: No registered users and 1 guest