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Anita O. Chemistry 101 5 months, 2 weeks ago
For empirical formula Step 1: Assume that the mass of a compound is 100 g. Step 2: Calculate the number of moles of each element. Step 3: Represent an empirical formula. Step 4: Divide the number of moles of each element by the least number of moles to get the subscripts of each element. Since the smallest number of moles is 3.41 mol, we divide each number of moles by 3.41 mol. Step 5: Multiply the subscripts obtained by a certain number to become whole number. Since the decimal part in 1.33 is 0.33, we need to multiply all the subscripts by 3. Therefore, Final Step: Write the empirical formula. Therefore, the empirical formula of ascorbic acid is C₃H₄O₃. -------------------------------------------------------- For molecular formula Step 1: Represent a molecular formula. Step 2: Calculate the empirical mass. Step 3: Divide the molecular mass by the empirical mass to find the value of n. Final Step: Multiply the subscripts by the value of n to obtain the molecular formula. Hence, the molecular formula of ascorbic acid is C₆H₈O₆. Note: Kindly swipe the screen to the left to see the continuation of the answers on the right side.#CarryOnLearning Rowan C.
vitamin C (absorbic acid) contains 40.92% C, 4.58%H , and 54.50 O ?? what is the empirical formula for vitamin C 1 Expert Answer When given % composition, and asked for the empirical formula, it is easiest to just assume 100 g of material. Thus, Mass C = 40.92 g. Moles C = 40.92 g x 1 mole/12 g = 3.41 moles C Mass H = 4.58 g. Moles H = 4.58 g x 1 mole/1.0 g = 4.58 moles H Mass O = 54.50 g. Moles O = 54.50 g x 1 mole/16 g = 3.41 moles O Next, we want to get the moles into whole numbers, so we begin by dividing all by the smallest, i.e. divide all by 3.41. Moles H = 4.58/3.41 = 1.34 Now, in order to get 1.34 to be a whole number we multiply it (and all others) by 3 Empirical Formula = C3H4O3 |