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Chapter 2: Q.31E (page 67)

Determine the empirical formula for the following compounds:

a) caffeine, C6H10N4O2

b) fructose, C12H22O11

c) hydrogen peroxide, H2O2

d) glucose, C6H12O6

e) ascorbic acid (vitamin C), C6H8O6

Short Answer

Expert verified

a) Empirical formula: C4H5N2O

b) Empirical formula: C12H22O11

c) Empirical formula: HO

d) Empirical formula: CH2O

e) Empirical formula: C3H4O3

Step by step solution

01

Step 1- Determine the definition of empirical formula

Empirical formula specifies the types of atoms present. It indicates the simplest whole-number ratio of the number of atoms (or ions) in the compound.

02

Step 2- Take out the common factor to determine the empirical formula.

caffeine=2 is the common factor, so the empirical formula will be C4H5N2O

fructose=no common factor. so the empirical formula will beC12H22O11

hydrogen peroxide =2 is the common factor, so empirical formula will be HO

glucose=6 is common factor, so empirical formula will be CH2O

ascorbic acid=common factor is 2, so empirical formula will be C3H4O3

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Most popular questions from this chapter

Write the molecular and empirical formulas of the following compounds:\(\begin{aligned}{}a)O = C = O\\b)H - C \equiv C - H\end{aligned}\)

c)

(d)

In what way are isotopes of a given element always different? In what way(s) are they always the same?

Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.

For each of the following pairs of ions, write the symbol for the formula of the compound they will form:

  1. \(C{a^{2 + }},{S^{2 - }}\)
  2. \(NH_4^ + ,SO_4^{2 - }\)
  3. \(A{l^{3 + }},B{r^ - }\)
  4. \(N{a^ + },HPO_4^{2 - }\)
  5. \(M{g^{2 + }},PO_4^{3 - }\)

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the 鈥淢ix Isotopes鈥� tab, hide the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� boxes, and then select the element boron.

(a) Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts.

(b) Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice.

(c) Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes fromtheir bins or click on 鈥淢ore鈥� and then move the sliders to the appropriate amounts.

(d) Reveal the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� boxes. How well does your mixture match withyour prediction? If necessary, adjust the isotope amounts to match your prediction.

(e) Select 鈥淣ature鈥檚鈥� mix of isotopes and compare it to your prediction. How well does your prediction comparewith the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match 鈥淣ature鈥檚鈥漚mounts as closely as possible.
See all solutions

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