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Chapter 3: Q 32E (page 169)

What information do we need to determine the molecular formula of a compound from the empirical formula?

Short Answer

Expert verified

If the empirical formula of a compound is known, then we can easily determine the molecular formula of the compound by the relation:

\({\rm{Molecular formula = n }} \times {\rm{ Empirical formula}}{\rm{.}}\)

Step by step solution

01

Empirical and molecular formula

The empirical formula and the molecular formula are related to each other but they are different in terms of formula. The simplest ratio of the elements present in a compound is given by the empirical formula of a compound, whereas the actual or original number of elements/atoms present in a compound is given by the molecular formula.

02

Relation between empirical and molecular formula

The relation between the molecular formula and the empirical formula of a compound is:

\({\rm{Molecular formula = n }} \times {\rm{ Empirical formula}}{\rm{.}}\)

Here, n is an integer whose value can be 1, 2, 3鈥�

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Most popular questions from this chapter

Question: Determine the following to four significant figures-

(a) The percent composition of hydrazoic acid, HN3

(b) The percent composition of TNT, C6H2CH3(NO2)3

(c) The percent of SO42- in Al2(SO4)3

A 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 g of HCl. What is the molarity of the solution?

D5W is a solution used as intravenous fluid. It is 5.0% by mass solution of dextrose C6H12O6 in water. If the density of D5W is 1.029g/ml. Calculate the molarity of dextrose in the solution.

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(a) 1.457 mol KCl in 1.500 L of solution

(b) 0.515 g of H2SO4 in 1.00 L of solution

(c) 20.54 g of Al(NO3)3 in 1575 mL of solution

(d) 2.76 kg of CuSO4鈭�5贬2O in 1.45 L of solution

(e) 0.005653 mol of Br2 in 10.00 mL of solution

(f) 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solution

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