Chemistry, 31.01.2020 15:51 PlzHelpMeOutKam2693

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

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Answer from: DarinKing2005

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.

$C_{3.407}H_{4.53}O_{3.406}\\\\C_\frac{3.407}{3.406}H_\frac{4.53}{3.406}O_\frac{3.406}{3.406}\\\\\\\boxed {C_1H_{1.33}O_1}$

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.

$3 \times \ C_1H_{1.33}O_1\\\\\boxed {\boxed {C_3H_4O_3}}$

LEARN MOREWriting Chemical Formula Naming Compounds Mole Conversion

Keywords: empirical formula, chemical formula

Answer from: Quest

1.consider the following balanced equation and answer parts a through. show calculations for each part.

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.

explanation:

Answer from: Quest

Idk the answer sorry

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