What is the empirical formula of ascorbic acid, given that the pseudoformula is c3.407 h4.53 o3.406? ?

The empirical formula of ascorbic acid is C₃H₄O₃. Empirical formula is the smallest whole number ratios of elements in a compound.  

FURTHER EXPLANATION

To get the empirical formula from mass percent data, the following steps are followed:

Get the mass percent data for all the elements that make up the compound.Assume that there is 100 grams of sample compound. Determine the equivalent masses of each element using the mass percent given.Convert the mass of each element to number of moles.Divide each calculated mole by the smallest mole value.The quotient will be the subscript of the element in the compound. If a decimal is obtained, round off the answers to the nearest whole number. Some exceptions to this are the following decimals: x.25, x.33, x.50, and x.75. When these decimals are obtained, all the subscripts are multiplied by a number that will result in a whole number.

Applying steps 1 to 3 to the problem leads to the pseudoformula C₃₋₄₀₇H₄₋₅₃O₃₋₄₀₆ where equivalent number of moles are written as the temporary subscripts of the elements in the compound.

STEP 4: Divide the moles by the smallest mole value which in this case is 3.406.

STEP 5: Multiply the subscripts by a number that would give the smallest whole number ratio.  

Since the decimal is 1.33 it cannot be automatically rounded off to 1. It should be multiplied by 3 to get the smallest whole number.

NOTE: All subscripts must be multiplied by the same factor, 3.

LEARN MOREWriting Chemical Formula Naming Compounds Mole Conversion

Keywords: empirical formula, chemical formula

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.

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