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Recall that the molecular formula of a compound is the actual molar ratio (ratio of moles) for each element.
For Vitamin A, the general molecular formula is given as: CxHyE, where E is an unknown element. Its molar mass is known to be: 286.4 g/mol, and it also contains 83.86% C, and 10.56% H by mass. We need to find the whole number values for x and y.
To solve for the molecular formula of Vitamin A we need to do these steps:
Vitamin A has a molar mass of 286.4 g/mol and a general molecular formula of C xHyE, where E is an unknown element. If vitamin A is 83.86% C and 10.56% H by mass, what is the molecular formula of vitamin A?
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Our tutors have indicated that to solve this problem you will need to apply the Empirical Formula concept. You can view video lessons to learn Empirical Formula. Or if you need more Empirical Formula practice, you can also practice Empirical Formula practice problems.
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Based on our data, we think this problem is relevant for Professor Lopreore's class at TULANE.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.