Nothing Special   »   [go: up one dir, main page]
Scribd Logo
Upload

Welcome to Scribd!

  • 174 views

    4th PPT Stoichiometry Empirical and Molecular Formula No Vid

    Uploaded by

    Wayne David C. Padullon
    The document discusses the difference between molecular and empirical formulas. An empirical formula gives the simplest whole number ratio of elements in a compound, while a molecular formula shows the actual number of each type of atom in a molecular unit of a compound. The document provides examples to illustrate how to calculate empirical formulas from elemental composition data and determine molecular formulas from empirical formulas and molecular masses.

    Copyright:

    © All Rights Reserved
    Download as PPTX, PDF, TXT or read online from Scribd

    4th PPT Stoichiometry Empirical and Molecular Formula No Vid

    Uploaded by

    Wayne David C. Padullon
    174 views14 pages
    The document discusses the difference between molecular and empirical formulas. An empirical formula gives the simplest whole number ratio of elements in a compound, while a molecular formula shows the actual number of each type of atom in a molecular unit of a compound. The document provides examples to illustrate how to calculate empirical formulas from elemental composition data and determine molecular formulas from empirical formulas and molecular masses.

    Original Description:

    Chemistry

    Original Title

    4th-PPT-Stoichiometry-Empirical-and-Molecular-Formula-no-vid

    Copyright

    © © All Rights Reserved

    Available Formats

    PPTX, PDF, TXT or read online from Scribd

    Did you find this document useful?

    Is this content inappropriate?

    The document discusses the difference between molecular and empirical formulas. An empirical formula gives the simplest whole number ratio of elements in a compound, while a molecular formula shows the actual number of each type of atom in a molecular unit of a compound. The document provides examples to illustrate how to calculate empirical formulas from elemental composition data and determine molecular formulas from empirical formulas and molecular masses.

    Copyright:

    © All Rights Reserved
    Download as PPTX, PDF, TXT or read online from Scribd
    Download as pptx, pdf, or txt
    174 views14 pages

    4th PPT Stoichiometry Empirical and Molecular Formula No Vid

    Uploaded by

    Wayne David C. Padullon
    The document discusses the difference between molecular and empirical formulas. An empirical formula gives the simplest whole number ratio of elements in a compound, while a molecular formula shows the actual number of each type of atom in a molecular unit of a compound. The document provides examples to illustrate how to calculate empirical formulas from elemental composition data and determine molecular formulas from empirical formulas and molecular masses.

    Copyright:

    © All Rights Reserved
    Download as PPTX, PDF, TXT or read online from Scribd
    Download as pptx, pdf, or txt
    of 14

    Molecular Formula VS.

    Empirical Formula
    What is a molecular formula?

    What is an empirical formula?

    What is the difference between the two?


    Molecular formula
     sometimes referred to as regular formula
     is actually how many atoms of each element are in a
    compound

    Empirical formula
     Gives the lowest whole number ratio of the atoms of the
    elements in a compound
    Molecular Formula Empirical Formula
    (ethene) C4H8 CH2
    (glucose) C6H12O6 CH2O
    C5H12 C5H12
    Small salad for 2 people
    1 Tbsp. vinegar : 3 Tbsp. olive oil
    Large salad for 4 people
    2 Tbsp. vinegar : 6 Tbsp. olive oil

    Empirical formula is the essential recipe!


    To calculate an empirical formula, we need to
    find the mole-mole ratio of the elements of the
    compounds.

    MOLE RATIOS MUST BE WHOLE


    NUMBERS!!!
    Example 1: Compound is 11.19% Hydrogen and
    88.81% Oxygen. Find the empirical formula.
    Example 2: Compound is 40.0% Carbon, 6.7%
    Hydrogen, and 53.3% Oxygen. Find the
    empirical formula.
    Example 3: DDT is 47.44% Carbon, 2.56%
    Hydrogen, and 50.0% Chlorine. Find the
    empirical formula.
    Example 4: Calculate the molecular formula of a
    compound when the empirical formula is C2H5.
    Its molecular mass is 58.0 g/mol.
    Group Drill
    1. 0.545g of Aluminum burns completely in
    Oxygen, producing 1.030g of aluminum oxide.
    Find the empirical formula of aluminum oxide.

    2. What is the molecular formula of a compound


    that is 85.7% Carbon and 14.3% Hydrogen by
    mass if the molecular mass is 28 g/mol?
    In your quiz notebook, answer the following questions:

    1-2. Differentiate molecular formula from empirical formula.


    (2 points)

    3-6. Determine the empirical formula of a compound that contains


    43.66% Manganese an 56.34% Chlorine. (4 points)

    7-10. Determine the molecular formula of a compound with the


    empirical formula CF2 and a molecular mass of 200.04 g/mol. (4
    points)

    You might also like