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in this problem being given an empirical formula of for Mula, um, of C two h four, and Oh, and we're told that the molar mass of the compound is 118.1 grams per mole. Now, we need to remember that an empirical formula is the most simplified version of a compounds molecular formula. So in order to find the molecular formula, we're gonna have to do a little bit of work here. First thing we want to do is figure out what is the molar mass of this substance here. So we're going to do two times 12.1 plus four times 1.8 plus 14.1 plus 16 point. Oh, so that we have the mess of all of those elements and we find that that comes out to be approximately 58.62 grams per mole, which obviously is less than the molar mass of the the substance we're working with. So what we're going to do now is we want to figure out what do you get closer to what the molecular formula is? Is we're gonna take this. I'm sorry. This is supposed to be 1 16 here. Not 1 18 1 16 Um, 116.1 grams per mole. Okay. And so what we're gonna do is going to take this 1 16.1 and divided by r 58.62 We find that that comes out to be approximately to, um, a little bit less. Um, but basically, because we need to use whole numbers, it comes up to, like 1.9995 etcetera. What's basically is to So we're gonna take this chemical formula normal empirical formula and multiply it by two to come up with our full, um, molecular formula. So our molecular tips is gonna be C four h eight and 202 So this is the molecular formula. This is the empirical formula, because again, the empirical is a simplified version of the molecular