Question

The molar mass and empirical formula of several compounds are listed here. Find the molecular formula of each compound. a. $\mathrm{C}_4 \mathrm{H}_9, 114.22 \mathrm{~g} / \mathrm{mol}$ b. $\mathrm{CCl}, 284.77 \mathrm{~g} / \mathrm{mol}$ c. $\mathrm{C}_3 \mathrm{H}_2 \mathrm{~N}, 312.29 \mathrm{~g} / \mathrm{mol}$

Name: Problem 68, Chapter 3: Principles of chemistry: A molecular approach
Uploaded: 2021-08-09T07:58:46-08:00
Duration: 3 min 16 s
Channel: Ma Ednelyn Lim
Description: The molar mass and empirical formula of several compounds are listed here. Find the molecular formula of each compound. a. C4 H9, 114.22 g / mol b. CCl, 284.77 g / mol c. C3 H2 N, 312.29 g / mol

   The molar mass and empirical formula of several compounds are listed here. Find the molecular formula of each compound.
a. $\mathrm{C}_4 \mathrm{H}_9, 114.22 \mathrm{~g} / \mathrm{mol}$
b. $\mathrm{CCl}, 284.77 \mathrm{~g} / \mathrm{mol}$
c. $\mathrm{C}_3 \mathrm{H}_2 \mathrm{~N}, 312.29 \mathrm{~g} / \mathrm{mol}$

Principles of chemistry: A molecular approach

Nivaldo J. Tro 3rd Edition

Chapter 3, Problem 68

Instant Answer

Solved by Expert Ma Ednelyn Lim

08/09/2021

Step 1

a. $C_4H_9$: Molar mass = (4 x atomic mass of C) + (9 x atomic mass of H) = (4 x 12.01 g/mol) + (9 x 1.01 g/mol) = 48.04 g/mol + 9.09 g/mol = 57.13 g/mol b. $CCl$: Molar mass = (1 x atomic mass of C) + (1 x atomic Show more…

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The molar mass and empirical formula of several compounds are listed here. Find the molecular formula of each compound. a. $\mathrm{C}_4 \mathrm{H}_9, 114.22 \mathrm{~g} / \mathrm{mol}$ b. $\mathrm{CCl}, 284.77 \mathrm{~g} / \mathrm{mol}$ c. $\mathrm{C}_3 \mathrm{H}_2 \mathrm{~N}, 312.29 \mathrm{~g} / \mathrm{mol}$

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Key Concepts

Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present. It is derived from the proportion of atoms in the compound, simplifying any common factors regardless of the actual number of atoms in a molecule.

Molar Mass

Molar mass is the mass of one mole of a substance expressed in grams per mole. It is obtained by summing the atomic masses of all atoms present in the molecular or empirical formula, enabling conversion between grams and moles.

Molecular Formula

The molecular formula gives the actual number of each type of atom in a molecule. It is determined by comparing the compound’s given molar mass to the molar mass of the empirical formula, using the ratio to scale up the empirical formula to the true molecular composition.

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